The following reaction increases the proportion of hydrogen gas for useas a fuel.CO(g) +H₂O(g) H2(g) + CO2(g)This reaction has been studied at different temperatures to find theoptimum conditions. At 700 K, the equilibrium constant is 8.3. Supposethat you start with 1.0 mol of CO) and 1.0 mol of H₂O(g) in a 5.0 Lcontainer. What amount of each substance will be present in thecontainer when the gases are at equilibrium, at 700 K?[Hint: Setup an I.C.E. table]Amount of CO at equilibrium:Amount of H₂O at equilibrium:Amount of H₂ at equilibrium:Amount of CO₂ at equilibrium:

Answered: Image /qna-images/answer/182e875e-df3a-49f9-a0ef-8c50ff370b63.jpg

The following reaction increases the proportion of hydrogen gas for use as a fuel. CO(g) + H₂O(g) → H2(g) + CO2(g) This reaction has been studied at different temperatures to find the optimum conditions. At 700 K, the equilibrium constant is 8.3. Suppose that you start with 1.0 mol of CO) and 1.0 mol of H₂O() in a 5.0 L container. What amount of each substance will be present in the container when the gases are at equilibrium, at 700 K? [Hint: Setup an I.C.E. table]

The following reaction increases the proportion of hydrogen gas for use as a fuel. CO(g) + H₂O(g) → H2(g) + CO2(g) This reaction has been studied at different temperatures to find the optimum conditions. At 700 K, the equilibrium constant is 8.3. Suppose that you start with 1.0 mol of CO) and 1.0 mol of H₂O() in a 5.0 L container. What amount of each substance will be present in the container when the gases are at equilibrium, at 700 K? [Hint: Setup an I.C.E. table]

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 3ALQ: For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each...

See similar textbooks

Similar questions

During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?
A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
Two molecules of A react to form one molecule of B, as in the reaction 2 A(g) B(g) Three experiments are done at different temperatures and equilibrium concentrations are measured. For each experiment, calculate the equilibrium constant, Kc. (a) [A] = 0.74 mol/L, [B] = 0.74 mol/L (b) [A] = 2.0 mol/L, [B] = 2.0 mol/L (c) [A] = 0.01 mol/L, [B] = 0.01 mol/L What can you conclude about this statement: If the concentrations of reactants and products are equal, then the equilibrium constant is always 1.0.
Consider the following equilibrium: COBr2(g) CO(g) + Br2(g)Kc = 0.190 at 73 C (a) A 0.50 mol sample of COBr2 is transferred to a 9.50-L flask and heated until equilibrium is attained. Calculate the equilibrium concentrations of each species. (b) The volume of the container is decreased to 4.5 L and the system allowed to return to equilibrium. Calculate the new equilibrium concentrations. (Hint: The calculation will be easier if you view this as a new problem with 0.5 mol of COBr2 transferred to a 4.5-L flask.) (c) What is the effect of decreasing the container volume from 9.50 L to 4.50 L?