An industrial chemist puts 1.05 mol each of H2(g) and CO2(g) in a 1.00-L container at a certain temperature. When equilibrium is reached, 0.72 mol of CO(g) is in the container. Find Keq at this temperature for the following reaction: H2(g) + CO2(g)↔H2O(g) + CO(g) Hint: Determine the expression for Keq (and notice that the answer will be unitless). For fixed T and V, remember that n will be proportional to P for ideal gases
An industrial chemist puts 1.05 mol each of H2(g) and CO2(g) in a 1.00-L container at a certain temperature. When equilibrium is reached, 0.72 mol of CO(g) is in the container. Find Keq at this temperature for the following reaction: H2(g) + CO2(g)↔H2O(g) + CO(g) Hint: Determine the expression for Keq (and notice that the answer will be unitless). For fixed T and V, remember that n will be proportional to P for ideal gases
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 56QAP: Sulfur oxychloride, SO2Cl2, decomposes to sulfur dioxide and chlorine gases. SO2Cl2(g)SO2(g)+Cl2(g)...
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An industrial chemist puts 1.05 mol each of H2(g) and CO2(g) in a 1.00-L container at a certain temperature. When equilibrium is reached, 0.72 mol of CO(g) is in the container.
Find Keq at this temperature for the following reaction:
H2(g) + CO2(g)↔H2O(g) + CO(g)
Hint: Determine the expression for Keq (and notice that the answer will be unitless). For fixed T and V, remember that n will be proportional to P for ideal gases
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