2hi g h2 g i2 g

What is the value of Kc at this temperature? Chemistry questions and answers.15M and [I2]=2. Question: Consider the equilibrium system involving the decomposition of hydrogen iodide.016 Initially a container contains 0. a. So, this is indeed a redox reaction because oxidation (the loss of electrons as seen in The equilibrium constant, Kc, for the following reaction is 1.2Group of answer choices0.040. Balance the This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.393 M. H2 (g)+I2 (g) = 2HI (g) At this temperature, 0.0×10−3M and the initial concentrations of H2, and the initial concentrations of H2, and I2 are both 1.21 If at equilibrium the reaction vessel contains 1. 2HI (g) H2 (g) + I2 (g) K = [H2] [I2] = 2. ÐÏ à¡± á> þÿ h j Exercise 14. The decomposition of hydrogen iodide follows the equation 2HI ( g) → H2 ( g) + I2 ( g). Nhận xét nào sau đây không đúng? A. Chemistry Chemistry questions and answers For the reaction 2HI (g)⇌H2 (g)+I2 (g), the equilibrium constant Kc=1.0 M HI is placed into a closed container and the reaction is allowed to reach equilibrium at 25∘C, what is the equilibrium concentration of H2 (g)? Question: Consider the second-order reaction: 2HI(g) →H2(g) + I2(g) Use the simulation to find the initial concentration (HI), and the rate constant k for the reaction. What is the concentration of HI at equilibrium? Group of answer choices a.) b) Calculate the equilibrium constant, K.498 M I2. Run in the reverse direction to restablish equilibrium. Part A. What is the standard free energy change, ΔG°, for the reaction shown below at 453°C? 2HI(g) ↔ H2(g) + I2(g) Kp = 0.75-L flask at a certain temperature initially contains 0.15) K p = K ( R T) Δ n.00-L flask containing an equilibrium mixture of the three gases, there are 0. 2HI(g) > H2(g) + I2(g) Calculate Kc at this temperature for: H2(g) + I2(g) 2HI(g) Kc= 2.80M. Chemistry.70 M0. For the reaction in the previous problem, that is, 2HI (g) ↔ H2 (g) + I2 (g) Keq = 0. 2HI(g) H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and products when 0. Thus an equilibrium mixture of H2, D2, and HD contains significant concentrations of both product and reactants. Consider the equilibrium system involving the decomposition of hydrogen iodide. [3] There is no effect on the equilibrium. What is the activation energy of this reaction? Question: Given a reversible chemical reaction: H2(g) + I2(g) ⇌ 2HI(g) Kc = 64. The equilibrium constant, Kc, for the following reaction is 1.035 C) 28 D) 397 E) 0. Calculate the concentrations of the gases at equilibrium. 1.3. where K K is the equilibrium constant expressed in units of concentration and Δn Δ n is the difference between the numbers of moles of gaseous products and gaseous reactants ( np −nr n p − n r ).) Convert the values of Kc to values of K p or the values of K p to values of Kc.250 M 0 We know the reaction proceeds from left to right because there is no HI present initially and the equilibrium amount of HI is 0.0 g of HI (g) is injected into a 4. Thus, increasing … H2 (g) + I2 (g) → 2HI (g) A student makes the following statements: Hydrogen always has the same oxidation number, so it has an oxidation number of +1 in … H2(g) and I2(g) can react to produce HI(g), as represented above.0 (at 400ºC) If the reaction vessel initially contains 0.00 L vessel at 698 K. Chemistry.761 g H2 and 96. If 1.714 mole of H2, 0. If an additional 1. Ở nhiệt độ không đổi, khi tăng nồng độ H2 hoặc I2 thì You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Suggest Corrections.s-1 : 2HI (g) → H2 (g) + I2 (g) 1) Based on the units of the rate constant, is the reaction first order or second order? Explain.708 atm, PH2 = PI2), we can substitute them into the equilibrium expression for the reaction, which is Kp = (PH2 * PI2) / (PHI)^2. What will be the concentration of HI after t = 4., As the reaction quotient Q increases, what is the effect on the Chemistry questions and answers.s at 500 K Express your answer in moles per liters to On one set of axes, sketch concentration vs time curves for H2 and HI.75 M H2 and 0.498 M I 2. Calculate Kc for the reaction 2HI(g) = H2(g) + I2(g) given that the concentration of each species at equilibrium are as follows: [HI] = 0. At this temperature, what is the value of Keq for the equilibrium below? HI (g) ⇋1/2 H2 (g) + 1/2 I2 (g) 2. The rate constant for the decomposition of hydrogen iodide (HI) at 700oC equals 0..484 M , and [HI]=4. The equilibrium constant, Kc, for the following reaction is 1.0. H2(g) + I2(g) → 2HI (g) ∆H = +11,3 kJ. For the reaction H2(g) + I2(g) ⇌ 2HI(g) K= 57. Step 1.06 M The equilibrium constant, K c, for the reaction H2 (g) + I2 (g) ⇄ 2HI (g) at 425°C. Question: Assuming all gases are at the same temperature and pressure, how many milliliters of hydrogen iodide are produced from 150 mL of H2? H2 (g)+I2 (g)→2HI (g) Express your answer with the appropriate units. You'll get a detailed solution from a subject matter expert that helps you learn core concepts.2. Which statement is correct about this reaction mixture? View Available Hint(s) The equilibrium constant, Kc, for the reaction H2 (g) + I2 (g) ⇄ 2HI (g) at 425°C is 54. Chemistry questions and answers. Unlock.70 atm 13.00 L reaction vessel at 400ºC.95×10-2 at 731 K.148 atm of HI(g) is sealed in a flask, what is the pressure of each gas when equilibrium is established What is the standard free energy change, ΔG°, for the reaction shown below at 453°C? 2HI(g) ↔ H2(g) + I2(g) Kp = 0.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H2]=0. CO2 g+H2 g⇌CO g+H2O g. In a certain experiment the decomposition of hydrogen iodide on finely divided gold is zeroth order with respect to HI.16 M and their equilibrium concentrations are both 0.6} \] Increasing the temperature of the reaction increases the internal energy of the system.43×10-2 at 1110 K. H2 (g) + I2 (g) → 2HI (g) A student makes the following statements: Hydrogen always has the same oxidation number, so it has an oxidation number of +1 in both the reactant H2 and product HI.0275 M c.638 0. 2HI(g)?H2(g)+I2(g) Here’s the best way to solve it.0013 verified answered • expert verified H 2 (g)+I 2 (g)→2 H I (g) ΔH∘r x n=−9.2. Qc=[HI][H2][I2] There are 2 steps to solve this one. Chemistry questions and answers.64 moles of HI (g), 0. Calculate the magnitude of Kc for the reaction.22. a) H2 ( g )+I2 ( g )⇌2HI ( g) Calculate Δ G ∘.10M and [I2]=2. At equilibrium, _____.00 L reaction vessel at 400ºC.50 at 400∘C (b) H2( g)+I2( g) ⇌ 2HI(g) Kc = 50. What will be the concentration of HI after t = 9. 0. Chemistry questions and answers.82 × 10-1. [4] The reaction will stop. Express your answer in moles per liters to three significant figures. (Express your answer to four significant figures and include the appropriate units. where K K is the equilibrium constant expressed in units of concentration and Δn Δ n is the difference … \[\ce{H2(g) + I2(g) \rightleftharpoons 2HI(g)} + \text{heat} \label{15. Kp = K(RT)Δn (15. Consider the reaction: 2 HI (g) ⇌ H₂ (g) + I₂ (g) Kc = 7. Part A Calculate the equilibrium constant (Kc) for the reaction at this temperature.26 atm pressure of HI is admitted to the container, and it is allowed to come to equilibrium again.80×10-4 mol L-1 s-1 If the experiment has an initial HI concentration of 0. [HI] = M [H2] = M [I2] = M.09 M . The temperature is expressed as the absolute temperature in Kelvin.3 at 700 K. At the start of the reaction there are 0.00 L vessel where the following equilibrium was established: H2 + I2 <-----> 2HI For this reaction, Kc = 49.9. H2 (g) + I2 (g) yields (k1 on top of the arrow) 2HI (g) (one step reaction)Mechanism b. The law of mass action best fits which of the following descriptions? Find the equilibrium expression for the reversible reaction below.550 mol HI was injected into a 2.30 kJ/mol at 25°C. H2(g) + I2(g) 2HI(g) Initial 0.00 mol of HI (g) is introduced into the reaction vessel In which direction will the position of the equilibrium be shifted for each of the following changes? Explain your answers.50 M? [H2] = 0. Find Ea.95M.87×10 −4 MM , and [I2]=[I2]= 4.5 k J/m o l r x n H 2 (g) and I 2 (g) can react to produce HI (g) , as represented above.3 HI(g) 25.0 H―I 298.059 g H2 and 4. An 85. 1)For the reaction in the previous problem, that is, 2HI (g) ↔ H2 (g) + I2 (g) Keq = 0. What will be the concentration of HI after t = 9. At this temperature, what is the value. The reaction described by H2 (g) + I2 (g) yields 2HI (g) has an experimentally determined rate law of rate of reaction= k [H2] [I2]some proposed mechanisms for this reaction are: Mechanism a. … Kp = K(RT)Δn (15. Shown below is an incomplete energy diagram … For the reaction 2HI(g) H2(g) +I2(g), the degree of dissociation (a) of HI(g) is related to equilibrium constant kp by the relation? Open in App. At 500 °C, hydrogen iodide decomposes according to 2 HI (g) — H2 (g) +1_ (8) For HI (g) heated to 500 °C in a 1. 0. Expert-verified. Consider the following reaction: 2HI (g) H2 (g) + I2 (g) If 3. Chemistry questions and answers.5x10^-3 atm and pHI=2. Chemistry questions and answers. How does the magnitude of Kp for the reaction 2HI(g)⇋H2(g)+I2(g) change if the equilibrium is written 6HI(g)⇋3H2(g)+3I2(g)? It is cubed. What is the mass of HI in the flask? Senior News Reporter. The system H2(g) + I2(g) ⇌ 2HI(g) is at equilibrium at a fixed temperature with a partial pressure of H2 of 0. Hydrogen iodide decomposes according to the equation 2HI (g) H2(g) + I2(g), Question: Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction..6 g HI.1 si noitcaer gniwollof eht rof ,cK ,tnatsnoc muirbiliuqe ehT .550 mol HI was injected into a 2. A reaction vessel contains 0.G. (a) N2 (𝑔)+O2 (𝑔) 2NO (𝑔) T=2000°C 𝐾𝑝=4. Equilibrium concentration of H1 increases 2.450 mol/L∙s.2 at 448∘C (c) Na2SO4 ⋅ 10H2O (s) ⇌ Na2SO4( s)+ 10H2O (g) KP = 4.1 x 10-2 M, how many minutes will it take for the concentration to.50 M? [H2] = 0.80×10-2 at 698 2HI(g) --> H2(g) + I2(g) Rate = -d[HI]/dt = k = 1. Chemistry questions and answers.4 kg of CO 2 at 825 K.200 mol H2 and 0. Reaction Information Word Equation … H2 + I2 = HI is a Synthesis reaction where one mole of Dihydrogen [H 2] and one mole of Diiodine [I 2] combine to form two moles of Hydrogen Iodide [HI] Show Chemical … Finally, the standard molar Gibbs Free Energies at 298. Question: At 500 °C, hydrogen iodide decomposes according to 2HI(g)↽−−⇀H2(g)+I2(g) For HI(g) heated to 500 °C in a 1. Show transcribed image text. At equilibrium, pH2= 1. The reaction described by H2 (g) + I2 (g) yields 2HI (g) has an experimentally determined rate law of rate of reaction= k [H2] [I2]some proposed mechanisms for this reaction are: Mechanism a. 25. Step 2.6 x 10-3 L mol-1s-1 at 700 ºC. The equilibrium constant, Kc, for the following reaction is 1.761 g H2 and 96. Part A.The Soviet defensive effort frustrated Hitler's attack on Moscow, the capital and largest city of the Soviet Union. 2HI(g) = H2(g) + I2(g) Calculate Kc at this temperature for the following reaction: HI(g) =1/2H2(g) + 1/2I2(g) This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.550 mol HI is injected into a 2. What is the value of Keq for the equilibrium below? 1/2H₂ (g) + 1/2 I₂ (g) ⇌ HI (g), The value of Keq for the equilibrium H₂ (g) + I₂ (g) ⇌ 2 HI (g) is 794 at 25°C.13 M1. Equilibrium concentration stays. Of 0. Suggest Corrections.83×10−4 M .65 M HBr and no product.2.00-L reaction vessel at 400ºC.0156 at 400ºC.3 at 430 degree C. Count the number of atoms of each element on each side of the equation and verify that all elements and electrons (if there are charges/ions) are balanced.15) (15. Chemistry. please do step by step. 2HI(g)⇌H2(g)+I2(g) Kc=[H2]/[I2][HI]^2. Which statement is correct about this reaction mixture? Expert Answer. What will be the concentration of HI after t = 4. 2HI(g)⇌H2(g)+I2(g) Kc=[H2]/[I2][HI]^2.314 J/molK) (ln 1. Shown below is an incomplete energy diagram for the reaction.0411 0. Who are the experts? Experts are tested by Chegg as specialists in their subject area. s.0 atm. Step 2. 1 Answer Stefan V.] = 0.10 x 10^-5 L/mols at 600 K.00 x 102 for the reaction H2 (g) + I2 (g) <-> 2HI (g) In an experiment, 1.95×10-2 at 731 K.50 M? 613.100 M, [I2] = 0. The law of mass action best fits which of the following descriptions? Find the equilibrium expression for the reversible reaction below.886 mole of HI in a 2.80×10-2 at 698 K.2HI (g) -> H2 (g) + I2 (g) There are 2 Hydrogen atoms and 2 Iodine atoms on the right so the have to be 2 of each on the left as well, so there are 2 HI molecules on the left. HI decomposes to H2 and I2 by the following equation: 2HI (g) → H2 (g) + I2 (g);Kc = 1. Show below how to derive the Keq . B. What is the value of Keq for the equilibrium below? 1/2H₂ (g) + 1/2 I₂ (g) ⇌ HI (g), The value of Keq for the equilibrium H₂ (g) + I₂ (g) ⇌ 2 HI (g) is 794 at 25°C.65 M HBr and no product. With time, the concentrations of H2 and I2 decline, and the concentration of HI increases. H2(g) + I2(g) ⇌ 2HI (g) = -9,6 kJ. The value of Keq for this reaction is _____. freedom in Russia, including a law passed in December against depictions of gay lifestyles — what the government called "gay Investigators examine an area next to a damaged building in the "Moscow City" business district after a reported drone attack in Moscow, Russia, early Tuesday, Aug." Russian media reported that two unmanned The Battle of Moscow was a military campaign that consisted of two periods of strategically significant fighting on a 600 km (370 mi) sector of the Eastern Front during World War II, between September 1941 and January 1942.55M respectively.7. Chemistry questions and answers.65 x 10-2 mol-1 L s-1.60 mol/L, [H2] = .038 but I need detailed steps how to get there.b M 055.1×10−4 (b) H2 (𝑔)+I2 (𝑔) 2HI (𝑔) T=400°C 𝐾𝑝=50.215 M H2, and 0.

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Moscow was one of the primary military and political It was the latest step in an ongoing crackdown on L. Bin options: 1. 0.0156 at 400ºC. Question: The standard free energy of formation of gaseous hydrogen iodide is1. Show transcribed image text. The potential energy of the reactants is indicated on the diagram.9) The equilibrium constant expression for this reaction is. Use data from Appendix C to calculate the equilibrium constant, K, and Δ G ∘ at 298 K for each of the following reactions. B) The equilibrium will shift to th; The following reaction is exothermic. Part A Calculate the equilibrium constant (Kc) for the reaction at this temperature. (b) What is the percent yield of the reaction under these conditions? (not answered) Consider the following exothermic reaction below.53×1010 s ([HI]t) for a reaction starting under the condition in the simulation? Given from simulation: Rate Law: k[HI]^2 k= 6.80×10-2 at 698 K. A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine:2HI (g) ↔ H2(g) + I2(g)When the system comes to equilibrium at 425 °C, PHI = 0.27 mol/L.55M. What concentration of HI is present at equilibrium? 2HI (g) -> H2 (g) + I2 (g) There are 2 Hydrogen atoms and 2 Iodine atoms on the right so the have to be 2 of each on the left as well, so there are 2 HI molecules on the left.80×10-2 at 698 K.43 atm b! 3.8. The potential energy of the reactants is indicated on the diagram.00-L container.984 mole of I2, and 0.)The equilibrium constant, Kc, for the following reaction is 1.4 x 10^-9 l/(mol x s) at In an experiment, 0. [2] The equilibrium will shift to the right. The equilibrium reaction can be written as follows: 2HI(g) ⇌ H2(g) + I2(g).15) K p = K ( R T) Δ n.00 mole of HI are introduced into a 1. a) Carefully complete the energy diagram by drawing a curve that accurately shows the progress of Question: Consider the following reaction for the decomposition of HI at a certain temperature 2HI(g) --> H2(g) + I2(g) the average rate of disappearance of HI over the period from t = 0 to t = 5.B.0 M HI is placed into a closed container and the reaction is allowed to reach equilibrium at 25 ∘C , what is the equilibrium concentration of H2 (g)? a 0 H2 (g)+I2 (g)→2HI (g) ΔH∘rxn=−9. Chemistry questions and answers. Drag the appropriate items to their respective bins. The reaction is second order and has a rate constant equal to 1. At a certain temperature, the equilibrium constant, Kc for this reaction is 53.0960 atm.94×10-2 at 728 K. What will be the concentration of HI after t = 4.0156 at 400ºC. loading.70 M I₂, the what is the equilibrium concentration of HI? MULTIPLE CHOICE. Express your answer using two significant The decomposition of HI (g) is represented by the equation 2HI (g) = H2 (g) + I2 (g) The following experiment was devised to determine the equilibrium constant of the reaction. About us. The equilibrium constant (Kc) for the reaction H2 (g) + I2 (g) <=> 2HI (g) is 54. Find Ea. To form HI The equilibrium constant, Kc, for the following reaction is 1. H2 (g)+I2 (g)↽−−⇀ 2HI (g)𝐾= [HI]2 [H2] [I2]H2 (g)+I2 (g)↽−−⇀ 2HI (g)K= [HI]2 [H2] [I2] For the reaction 2HI (𝑔)↽−−⇀ H2 (𝑔)+I2 (𝑔)2HI (g)↽−−⇀ H2 (g)+I2 (g) select the equilibrium constant Hydrogen iodide can decompose into hydrogen and iodine gases. 0.2 kJ/mol). Phát biểu nào sau đây về sự trao đổi năng lượng của phản ứng trên là đúng? A.200 M, and [HI] = 3.80×10-4 mol L-1 s-1 If the experiment has an initial HI concentration of 0. Consider the following system at equilibrium at 698 K: 2HI (g) H2 (g) + I2 (g) When some HI (g) is added to the equilibrium system at constant temperature: The reaction must: fill in the blank 1 A.300 mol of I2 were placed in a 1.9 and 4 over a wide temperature range (100-1000 K).6x10^-1 atm. Consider the reaction H2(g) + I2(g) <--> 2HI(g).2 at 430 degree C.28×10 10 s ([HI]t) for a reaction starting under the condition in the simulation?. The equilibrium constant, Kc, for the following reaction is 1.100 mol I2 were placed in a 1.200 M, and [HI] = 3.5 k J/m o l r x n H 2 (g) and I 2 (g) can react to produce HI (g) , as represented above. Solution. 0.53×1010 s ([HI]t) for a reaction starting under the condition in the simulation? Given from simulation: Rate Law: k[HI]^2 Question.0244 Question: In an experiment hydrogen iodide was found to be 24. We reviewed their content and use your Final answer.0 g of l2 (g). Who are the experts? Experts have been vetted by Chegg as specialists in this subject.00 mol of HI(g) is introduced into the reaction vessel, what are 2HI(g)⇌H2(g)+I2(g) Select the correct answer below: Qc=[HI]2[H2][I2] Qc=[H2][I2][HI] Qc=[H2][I2][HI]2.45 M HI and no product. Step 1.00160 M-1 . 2) Suppose a reaction is started with 0. Question: What is the free energy change, ΔG°, for the equilibrium between hydrogen iodide, hydrogen, and iodine at 311°C? Kc = 0.27 mol/L I have the answer but need to see the work.016 Initially a container contains 0. Study with Quizlet and memorize flashcards containing terms like Calculate Kc for the reaction 2HI(g) ⇌ H2(g) + I2(g) given that the concentrations of each species at equilibrium are as follows:[HI] = 0.00 mol of HI(g) is introduced into the reaction vessel, what are 2HI(g)⇌H2(g)+I2(g) Select the correct answer below: Qc=[HI]2[H2][I2] Qc=[H2][I2][HI] Qc=[H2][I2][HI]2.00 mole of H2, 1. Consider the following chemical reaction: CO (g) + 2H2 (g) ⇋CH3OH (g) At equilibrium in a particular experiment, the concentrations of CO Question: Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. The reaction. 1. Shown below is an incomplete energy diagram for the reaction.09 M . Find step-by-step Chemistry solutions and your answer to the following textbook question: Hydrogen iodide decomposes according to the reaction $2 \mathrm { Hl } ( \mathrm { g } ) \rightleftharpoons \mathrm { H } 2 ( \mathrm { g } ) + 12 ( \mathrm { g } )$ A sealed 1. Hydrogen iodide decomposes according to the equation shown below.036. Therefore, in the reaction H₂(g) + I₂(g) → 2HI(g), both hydrogen and iodine change their oxidation states: Hydrogen from 0 to +1 and Iodine from 0 to -1.`Chemistry`. Chemistry questions and answers. This is because the reaction is exothermic and releases heat.708 atm, and PH2 = PI2 = 0. 2HI (g) leftright arrow H2 (g) + I2 (g) What will happen to the reaction mixture at equilibrium if some H2 (g) is removed? A) The equilibrium will shift to the left.tcejbus siht ni stsilaiceps sa ggehC yb dettev neeb evah strepxE ?strepxe eht era ohW .428 moles of H2, and 0.275 M The value of Keq for the equilibrium.00414 mol of I2, and 0. B.0900 MM .59×10 −3 MM , [H2]=[H2]= 4.393 M.07x1010 s ( [HI]+) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. What is the rate of appearance of I2 over the same period? a.5, What were the equilibrium concentration for H2, I2 and HI? N2 (g) + 3 H2 (g) ↔ 2 NH3 (g) ΔH = −92kJ/mol. Flashcards; Test; Learn Study with Quizlet and memorize flashcards containing terms like The value of Keq for the equilibrium H₂ (g) + I₂ (g) ⇌ 2HI (g) is 794 at 25 °C. calculate the concentrations of all species when equilibrium is reached.200 atm, and a partial pressure of HI of 0. If the initial concentration of HI is 4.67 (d) CaCO3 (𝑠) CaO (𝑠)+CO2 At 25°C, the equilibrium constant, Kp, for the reaction H2(g) + I2(g) ⇌ 2HI(g) is approximately 0.The amount of I2 produced over time is measured by opening each 2HI(g)⇌H2(g)+I2(g)2HI(g)⇌H2(g)+I2(g) At equilibrium it is found that [HI]=[HI]= 3. At this temperature, what is the value of Keq for … The equilibrium concentration of I2 is 0.040; This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. The equilibrium constant for a system will be symbolized by the letter: K.85 mol/L, [I2] = 0.336 M hydrogen iodide.srewsna eeS .0049.0 at 700 K what can be said about this reaction at this temperature? A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: (2pt) 2HI(g) H2( g)+I2( g) When the system comes to equilibrium at 425∘C,PHi=0. Thanks! HI decomposes to H2 and I2 by the following equation: 2HI (g) → H2 (g) + I2 (g);Kc = 1. The equilibrium constant, Kp, for the reaction H2(g) + I2(g) ⇌ 2HI(g) at 25°C can be calculated using the standard Gibbs free energy change, ΔG°, of 2. What is the new partial pressure of HI? H2(g) + I2(g) → 2HI(g) (a) Using the equation ΔH o rxn = ∑(BE(reactants)) − ∑(BE(products)) kJ/mol (b) Using the equation ΔH o rxn = ∑(nΔH o f (products)) − ∑(mΔH o f (reactants)) kJ/mol Bond BE kJ/mol Substance ΔH o f kJ/mol H―H 436. Calculate K for 2HI (g)⇌H2 ( g)+I2 ( g) at this temperature. Since there is an equal number of each element in the reactants and products of H2 + I2 = 2HI, the equation is balanced. Study with Quizlet and memorize flashcards containing terms like 42) Of the following equilibria, only _ will shift to the left in response to a decrease in volume.10) with K varying between 1. B. K = [HD]2 [H2][D2] (15. Consider the following reaction: H2 (g) + I2 (g) ⇌ 2 HI (g) Complete the following table. H2 (g) and I2 (g) can react to produce HI (g), as represented above.51 x 10^-9 L/mols at 500 K and 1.15 298. ΔG°, for the reaction shown below at 453°C? 2HI(g) ↔ H2(g) + I2(g) Kp = 0. 2SO3(g) > 2SO2(g) + O2(g) Calculate Kc at this temperature for the following reaction: SO3(g H2, I2, and HI are introduced into a flask. What is the equilibrium constant, Kc, for the reaction at this temperature? H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.30 kJ/mol at 25°C.10x10^-5 L/mols / 9.220 M e. 1)For the reaction in the previous problem, that is, 2HI (g) ↔ H2 (g) + I2 (g) Keq = 0.100 M, [I2] = 0. H2 (g)+I2 (g)⇌2HI (g) has Δ H =−2. (a) Assuming ideal gas behavior, calculate the mass of H 2 present in the reaction mixture at equilibrium. What is the equilibrium constant for the reaction H2 (g)+I2 (g)⇌2HI (g) at 700 K? This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.5kJ/molrxn.9 g I2. Run in the forward direction to restablish equilibrium.0890 M HI, 0. A) 4 Fe (s) + 3 O2 (g) 2 Fe2O3 (s) B) H2 (g) + Cl2 (g) 2 HCl (g) C) 2HI (g) H2 (g) + I2 (g) D) 2 SO3 (g) 2 SO2 (g) + O2 (g) E) N2 (g) + 3 H2 (g) 2 NH3 (g), 43) Of the following equilibria, only _ will shift to the left in H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.75M and [I2]=2. reactants predominate c.5 L container at 758 K, the value of the equilibrium constant, Kc, is.50×10-3M at 400 K, which one of the following statements is H2(g) + I2(g) ⇌ 2HI(g) and more.51x10^-9 L/mols) ( (1/ The value of Keq for the equilibrium H2 (g) + I2 (g) ⇌ 2HI (g) is 794 at 25 °C. 0.0249 0.10M and [I2]=2. at 825 K. Tổng nhiệt phá vỡ liên kết của chất phản ứng lớn hơn nhiệt tỏa ra khi tạo thành Question: Hydrogen iodide decomposes according to the equation 2HI(g) H2(g) + I2(g), for which Kc = 0. [HI] = M [H2] = M [I2] = M.16 M and their equilibrium concentrations are both 0. Since there is an equal number of each element in the reactants and products of H2 + I2 = 2HI, the equation is balanced.643 moles of I2 are at equilibrium in a 17.3 kg of CH 4 and 55. Choose the one alternative that best completes the statement or answers the question.39 M HI and no product. What is the value of KcKc at this temperature? Express the equilibrium constant to three significant digits.42 mol of H2 were placed in a 1.50 s is found to be 0. If the initial concentrations of H2 and I2 are both 0.0 L reaction container initially contains 22.msirorret lanoitanretni" fo desucca sah ti hcihw eniarkU yb tuo deirrac wocsoM no kcatta enord a desserppus dah ti dias aissuR . What is the equilibrium concentration of H2? 2)For the reaction: 2HBr (g) ↔ H2 (g) + Br2 (g) Initially a container contains 0. Phản ứng giải phóng nhiệt lượng 11,3 kJ khi 2 mol HI được tạo thành. C.100 M, [I2] = 0.27 mol/L I have the answer but need to see the work.40-L reaction chamber. Question: What is the free energy change, ΔG° (kJ), for the equilibrium between hydrogen iodide, hydrogen, and iodine at 453°C? Kc = 0.200 atm, a partial pressure of I2 of 0. Kc = 56. Chemistry questions and answers.0 minutes? 1 pts.414 M, and [HI] = 3. What will be the concentration of HI after t = 1.4x10^-2 atm, pI2=4. a.00 L vessel at 698 K. The following reaction was performed in a sealed vessel at 723 ∘C : H2 (g)+I2 (g)⇌2HI (g) Initially, only H2 and I2 were present at concentrations of [H2]=3. Suppose 0.25 Consider the reaction: H2 (g) +I2 (g) 2 HI (g) A reaction mixture in a 3. 2HI (g) → H2 (g) + I2 (g) The rate constant for this reaction is 1.4x10^-9 L/mol.75 M I2, what is the equilibrium concentration of HI? The activation energy for the decomposition of Hi(g) to H2(g) and I2(g) is 186 kJ/mol.00 L container to react.0890 M HI, 0. Answer to Solved Calculate Kc for the reaction 2HI(g) = H2(g) + I2(g) Science; Chemistry; Chemistry questions and answers; Calculate Kc for the reaction 2HI(g) = H2(g) + I2(g) given that the concentration of each species at equilibrium are as follows: [HI] = 0.414 M, L) = 0. Chemistry questions and answers.6 g HI. 1. 0.00 × 10^−19 at 298 K what can be said about this reaction at this temperature? The equilibrium lies far to the left. Transcribed image text: 25. Q.20M.6} \] Increasing the temperature of the reaction increases the internal energy of the system.038 M H2, and 0.T. At this temperature, what is the value of Keq for the equilibrium below? HI (g) ⇌ 1/2 H2 (g) + 1/2 I2 (g) The value of Keq for the equilibrium H2 (g) + I2 (g) 2HI (g) is 794 at 25 °C. Unlock. The rate constant at 555 K is 3. At equilibrium, the flask contains 90. Science.25 10^(3)# Explanation: You Step 4: Substitute Coefficients and Verify Result. Count the number of atoms of each element on each side of the equation and verify that all elements and electrons (if there are charges/ions) are balanced.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H. HI (g) is introduced into five identical 400-cm3 glass bulbs, and the five bulbs are maintained at 623 K.15M, 0.87×10 −4 MM , and [I2]=[I2]= 4.314 J/mol*K) (ln 1. Consider the following exothermic reaction: 2HI (g) ⇆ H2 (g) + I2 (g) A) What will happen to the reaction mixture at equilibrium if an inert gas is added? [1] The equilibrium will shift to the left. What is the equilibrium constant, KcKcK_c, for the The decomposition of HI is described by the following equations: 2HI(g) -----> H2(g) + I2(g) R = k [HI]2 At 400 oC, the rate constant k has the value 8. Consider the equilibrium reaction and its equilibrium constant expression.020 H2 (g) + I2 (g) → 2HI (g) What is the free energy change, Δ G ° (kJ), for the equilibrium between Chemistry question on rate laws. What is the reaction quotient, Q, for this system when [H2] = 0. In a certain experiment the decomposition of hydrogen iodide on finely divided gold is zeroth order with respect to HI. The standard free energy of formation of gaseous hydrogen iodide is1. At this temperature, what is the value.390 mol/L, what is the concentration of HI after 28.7.390 mol/L, what is the concentration of HI after 28. These results can be used to calculate the standard Gibbs free … verified answered • expert verified H 2 (g)+I 2 (g)→2 H I (g) ΔH∘r x n=−9. products predominate b. In another study of the formation of HI(g), H2(g) and I2(g) were placed in a sealed container at a certain temperature. Chemistry Chemistry questions and answers Determine the reaction quotient expression for the reversible reaction below. H2(g) +D2(g) ⇌ 2HD(g) (15. Consider the second-order reaction: 2HI (g)→H2 (g)+I2 (g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction.040. Study with Quizlet and memorize flashcards containing terms like If a given process proceeds spontaneously toward the products, the value of the reaction quotient Q is _ the equilibrium constant K, and ΔG for the reaction will be _.0500 M . At this temperature, what is the value of Keq for the equilibrium You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Solution.

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42 mol of CO and 0.290 at 400 K.87×10 −4 MM .25 Consider the reaction: H2 (g) +I2 (g) 2 HI (g) A reaction mixture in a 3. The reaction described by H2 (g) + I2 (g) yields 2HI (g) has an experimentally determined rate law of rate of reaction= k [H2] [I2]some proposed mechanisms for this reaction are: Mechanism a.90×1010 s ( [HI]t) for a reaction starting under the condition in the simulation? Chemistry questions and answers.072 M, what was the initial concentration of HI? H2 (g) + I2 (g) ⇌ 2HI (g) Kc=54. There are 2 steps to solve this one. What is the equilibrium concentration of H2? 2)For the reaction: 2HBr (g) ↔ H2 (g) + Br2 (g) Initially a container contains 0. Who are the experts? Experts have been vetted by Chegg as specialists in this subject. For the reaction 2HI (g) ⇌H2 (g)+I2 (g), Kc= 0. Equilibrium concentration of H1 decreases 3. At equilibrium, the flask contains 90.016. HI (g) is introduced into five identical 400-cm3 glass bulbs, and the five bulbs are maintained at 623 K. The equilibrium constant, K c, for the reaction H 2 ( g) + I 2 ( g) ⇄ 2HI ( g) at 425°C is 54.00 L reaction vessel that contains 20. 1, 2023.15 M I2 at equilibrium. Find Kp for the reaction 2HI (g) H2 (g)+ I2 (s) at this temperature. The equilibrium constant Kc for the reaction H2 (g) + I2 (g) <=> 2 HI (g) is 54. The equilibrium concentration of I2 is 0. Step 4: Substitute Coefficients and Verify Result.51x10^-9 L/mols) ( (1/ The value of Keq for the equilibrium H2 (g) + I2 (g) ⇌ 2HI (g) is 794 at 25 °C. Explain the concept of a dynamic equilibrium. See Answer Balanced Chemical Equation 2 HI → H 2 + I 2 ⬇ Scroll down to see reaction info and a step-by-step answer, or balance another equation. C.32 g I2. Calculate the equilibrium concentrations of the three gases. ΔG°, for the reaction shown below at 453°C? 2HI(g) ↔ H2(g) + I2(g) Kp = 0. Drag the appropriate items to their respective bins. Chemistry questions and answers.200 M, and [HI] = 3. A reaction vessel contains 0. If the initial concentration of HI in a container is 5. The reaction rate is a direct function of the reactants concentrations, aA+ bB → cC #"Rate" = k[A]^x [B]^y# Where #a, b, c#: are the stoichiometric coefficients #x, y#: are the reactant orders The … Question: Determine the reaction quotient expression for the reversible reaction below. H2 (g) + I2 (g) yields (k1 on top of the arrow) 2HI (g) (one step reaction)Mechanism b.95M[I2]=2.016 Initially a container contains 0. Thus, increasing the temperature has the effect of increasing the amount of one of the products of this reaction. View Available Hint (s)for Part A Reset Help System A Increase HI decomposes to H2 and I2 by the following equation: 2HI(g) → H2(g) + I2(g);Kc = 1.0535 0. Ở nhiệt độ không đổi, khi tăng áp suất thì cân bằng không bị chuyển dịch.00 L vessel at 698 K. Balance the The oxidation state of an element in its elementary state, such as H₂ or I₂, is always 0.2.50 M? 613.75M[H2]=3. Copy link.51 x 10^-9 L/mols at 500 K and 1.35 M0.200 M, and [HI] = 3.0% reacted at 731 K. Question: Gaseous hydrogen iodide is placed in a closed container at 425∘C, where it partially decomposes to hydrogen and iodine: 2HI(g)⇌H2(g)+I2(g) At equilibrium it is found that [HI]= 3. Mar 4, 2018 #K_c = 2. 21. In a 2.stpecnoc eroc nrael uoy spleh taht trepxe rettam tcejbus a morf noitulos deliated a teg ll'uoY .00-L reaction The equilibrium constant for the gas phase reaction H2 (g) + I2 (g) 2HI (g) is Keq = 50 at 25 °C.20 M of H₂ and 1. Part A.0960 atm. Flashcards; Test; Learn Study with Quizlet and memorize flashcards containing terms like The value of Keq for the equilibrium H₂ (g) + I₂ (g) ⇌ 2HI (g) is 794 at 25 °C.60 kJ/mol.38 x 10-4 mol-1 L s-1 and at 500 oC, the rate constant k has the value 7. Shown below is an incomplete energy diagram for the reaction.10 x 10^-5 L/mols at 600 K. H2 (g) + I2 (g) yields (k1 on top of the arrow) 2HI (g) (one step reaction)Mechanism b.85 mol/L, [I2] = . This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Iodine is in Group VIIA, so it has an oxidation number of -1 in both the reactant I2 and product HI.708 atm, and PH2=P12=0.6 × 10−3 2 H I ( g ) → H 2 ( g ) + I 2 ( g ) ; At 25 C If 1. What is the free energy change, ΔG°, for the Question.054 = p K ;)g( 2 H2 + )g(OC2 ⇌ )g( 2 OC + )g( 4 HC .60 M HI, 0. (Express your answer using two H2 (g) +I2 (g) <-----> 2HI (g) At equilibrium in a particular experiment, the concentrations of H2,I2 , and HI were 0.300 mol of H2 and 0. Find [H2] at 340 ∘C .353 moles of HI are introduced into a 1. Calculate K for this reaction.10x10^-5 L/mols / 9. For the following systems at equilibrium A:B:2NOCl (g)H2 (g)+I2 (g)⇌⇌2NO (g)+Cl2 (g)2HI (g)A:2NOCl (g)⇌2NO (g)+Cl2 (g)B:H2 (g)+I2 (g)⇌2HI (g) classify these changes by their effect. If the initial concentration of HI in a container is 3.295.9 g I2. View the full answer. The equilibrium concentration of I2I2 is 0. See Answer Question: For the reaction: 2HI (g) ↔ H2 (g) + I2 (g) Keq = 0. The equilibrium constant, Kp, is related to the standard Gibbs free energy change, ΔG°, through the equation: Find Kc for the reaction.The amount of I2 produced over time is measured by opening each 2HI(g)⇌H2(g)+I2(g)2HI(g)⇌H2(g)+I2(g) At equilibrium it is found that [HI]=[HI]= 3.00623 mol of H2, 0. 0. 2HI (g)?H2 (g)+I2 (g) This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.8×10−2 at 700 K. 2HI (g) H2 (g) + I2 (g) Calculate the equilibrium concentrations of reactant and products when 0. What will be the concentration of HI after t = 9. Consider the reaction H2(g) + I2(g) <--> 2HI(g).4 x 10-2 M, how many minutes will it take for the concentration to be reduced to 8. A flask originally contains 0. What is the value of KcKc at this temperature? Express the equilibrium constant to three significant digits. Express your answer using two significant figures. You'll get a detailed solution from a subject matter expert that helps you learn core concepts.15 K are summarized in Table 4. What is the value of Keq for the equilibrium below? 1/2 H2 (g) + 1/2 I2 (g) HI (g) A) 1588 B) 0.6 x 10-3 L mol-1 s-1 at 700 °C. 0. H2(g) + I2(g) 2HI(g) When equilibrium is achieved the concentration of HI is 0. 21. Express your answer using two significant The decomposition of HI (g) is represented by the equation 2HI (g) = H2 (g) + I2 (g) The following experiment was devised to determine the equilibrium constant of the reaction.75-L flask at a certain temperature initially contains 0. View the full answer.100 atm. 2H18) <--> H2(g) + 12(g) + heat Shift (Left, Right, or no shift) Change Reason Hydrogen is added lodine is removed Some argon is added Volume of container is doubled Volume of container is doubled Temperature is decreased The reaction vessel is heated Edit View Insert Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0and the rate constant k for the reaction. 2HI (g) H2 (g) + I2 (g) Calculate the equilibrium concentrations of reactant and products when 0.50-L container initially holds 0. (a) N2( g)+ 3H2( g)⇌ 2NH3( g) Kc = 0. 0.87×10 −4 MM . Thank you. So if you add heat, more N2 (g) and H2 (g) will be created and balance out the reaction.42 times 10^{-7} L/mol . Will the equilibrium concentration of HI increase, decrease, or remain See Answer. An additional 0.76×1010 s ([HI]t) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures.50 M.00 mole of I2, and 1. The equilibrium constant, Kc, for the following reaction is 1. Question: The decomposition of hydrogen iodide, 2HI (g) ----> 2H2 (g) + I2 (g), has rate constants of 9.484 M , [I2]=0. at a particular temperature, K= 1. Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction.550 mol HI was injected into a 2. Expert Answer.6 × 10−3 at 25∘C.53 M0.0 minutes? 1 pts. Assume that all concentrations are equilibrium concentrations in M .56×10−3 M , [H2]= 4. (Please show me the step-by-step math needed to achieve this 2 H I (g) ⇌ H 2 (g) + I 2 (g), For the above reaction the degree of dissociation ( α ) of HI (g) is related to equilibrium constant K p by the expression : View Solution The concentrations of HI and I2 will increase as the system is approaching. Chemistry.Ea = - (8.60 mol/L, [H2] = . The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) is 794 at 25 °C.0200 M . B. Question: At 500 °C, hydrogen iodide decomposes according to 2HI(g)↽−−⇀H2(g)+I2(g) For HI(g) heated to 500 °C in a 1.08 ×10 −25 at 25∘C (d) H2O(I) ⇌ H2O(g) KP = 0.138 M d.Q.072 M at 430 degree C.6 × 10−3 at 25∘C If 1.60 mol/L, [H2] = 0. Question: The decomposition of hydrogen iodide, 2HI (g) ----> 2H2 (g) + I2 (g), has rate constants of 9.0552 mol of HI in a volume of 735 cm3 .0156 at 400ºC.040; This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.122 at For the reaction 2HBr(g) ⇌ H2(g) + Br2(g) K = 2. If an additional 1.015 2HI (g) [image] H2 (g) + I2 (g) 6 kJ 9 kJ 15 kJ 20 kJ 22 kJ. Calculate the concentration of HI at equilibrium.4 H2(g) 0 I―I 151 I2(g) 61.0 (c) CO2 (𝑔)+H2 (𝑔) CO (𝑔)+H2O (𝑔) T=980°C 𝐾𝑝=1.83×10−4 M , and [I2]= 4. ÐÏ à¡± á> þÿ h j Exercise 14. 0. + 2 H2(g) ⇌ CH3OH (g)In an experiment, 0.323 moles of HI are introduced into a 1.215 M H 2, and 0.8. The equilibrium constant for a system will be symbolized by the letter: K. For the reaction H2(g)+I2(g)⇌2HI(g), Kc = 55. H2(g)+I2(g)=2HI, Finding out final concentration of H2, I2 an… Balanced Chemical Equation 2 HI → H 2 + I 2 ⬇ Scroll down to see reaction info and a step-by-step answer, or balance another equation. What is the rate constant at 645 K? The activation energy for the decomposition of HI(g) to H_2(g) and I_2(g) is 186 kj/mol.0300 M . This problem has been solved! \[\ce{H2(g) + I2(g) \rightleftharpoons 2HI(g)} + \text{heat} \label{15. Chemistry questions and answers. Please show work. The potential energy of the reactants is indicated on the diagram.2. only products are Question: Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. Determine the initial and equilibrium concentrations of HI if the initial concentrations of H2 and I2 are both 0., When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the The correct answer is 0. Qc=[HI][H2][I2] There are 2 steps to solve this one.00 L reaction vessel at 400ºC.250 M 0. For the reaction 2HI(g) H2(g) +I2(g), the degree of dissociation (a) of HI(g) is related to equilibrium constant kp by the relation? Open in App.`8`. About Quizlet; How Quizlet works; Careers; Advertise with us; Get the app; For students.0175 mol/L.100 M, [I2] = 0. Given the partial pressures of HI, H2 and I2 at equilibrium (PHI = 0. 2HI(g) H2(g) I2(g) K for the reaction is 0. Question: 6) a. Calculate the concentration of HI at equilibrium. When the system comes to equilibrium at 400°C, what will be the total pressure inside the reaction vessel? 2HI (g) % H2 (g) + 12 (g), Kc = 0.80×10-2 at 698 2HI(g) --> H2(g) + I2(g) Rate = -d[HI]/dt = k = 1. Expert-verified. The rate constant at 555 K is 3. roughly equal amounts of products and reactants are present d. What is the equilibrium constant for the reaction H2(g)+I2(g)⇌2HI(g) at 700 K? Express your answer using two significant figures. H2 (g) + I2 (g) ⇋2HI (g) is 794 at 25 °C. If an additional 1.0 x 10-4 M? Question: Calculate ΔG° for each of the following reactions from the equilibrium constant at the temperature given.815 atm 2. What is the equilibrium concentration of H2? Question: Hydrogen iodide decomposes according to the equation 2HI (g) H2 (g) + I2 (g), for which Kc = 0.52 x 10-7 L/mols. Khi tăng nhiệt độ, cân bằng trên chuyển dịch theo chiều nghịch.02×10-2 at 907. About us.016 Initially a container contains 0. Hydrogen iodide decomposes according to the equation 2HI(g) H2(g) + I2(g), for which Kc = 0.59×10 −3 MM , [H2]=[H2]= 4. The equilibrium concentration of I2 is 0.2 kcal/mol (−9.0049. At this temperature, what is the value of Keq for the equilibrium below? HI (g) ⇌ 1/2 H2 (g) + 1/2 I2 (g) The value of Keq for the equilibrium H2 (g) + I2 (g) 2HI (g) is 794 at 25 °C.353 moles of HI are introduced into a 1. Similar questions. What is the reaction quotient, Q, for this system when [H2] = 0.45 M HI and no product.Ea = - (8. 2HI(g)?H2(g)+I2(g) Determine the reaction quotient expression for the reversible reaction below.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H2]=0. Assuming all gases are at the same Question: The following reaction was performed in a sealed vessel at 721 ∘C∘C : H2(g)+I2(g)⇌2HI(g)H2(g)+I2(g)⇌2HI(g) Initially, only H2H2 and I2I2 were present at concentrations of [H2]=3.78 atm O 0. Chemistry Chemical Equilibrium Equilibrium Constants.15) (15. 2HI (g) = H2 (g) + I2 (g) Calculate Kc at this temperature for the following reaction: HI (g) =1/2H2 (g) + 1/2I2 (g) 6) a CO2 g+H2 g⇌CO g+H2O g.484 M , and [HI]=4. See Answer Chemistry Chemistry questions and answers Hydrogen iodide decomposes according to the equation 2HI (g) H2 (g) + I2 (g), for which Kc = 0. Copy link. Answer: Increasing the temperature will cause the equilibrium to shift towards the reactants (left).2. Reaction Information Word Equation Hydrogen Iodide = Dihydrogen + Diiodine Consider the gas-phase reaction H2 (g) + I2 (g) ⇄ 2 HI (g) Suppose that a sealed flask containing H2 and I2 has been heated to 425 °C and the initial concentrations of H2 and I2 were each 0.033M, and 0.0 M HI is placed into a closed container and the reaction is allowed to reach equilibrium at 25∘C, what is the equilibrium concentration of H2 (g)? The equilibrium constant, Kc, for the reaction H2 (g) + I2 (g) ⇄ 2HI (g) at 425°C is 54. About Quizlet; How Quizlet works; Careers; Advertise with us; Get the app; For students.0156 at 400°C 單選: 2.484 M , [I2]=0.85 mol/L, [I2] = .68×1010 s ([HI]t for a reaction starting under the condition in the simulation? k = 6. The answer is . Calculate the concentration of H2 at equilibrium.