Suppose a 250. mL flask is filled with 0.80 mol of H₂O, 0.50 mol of CO₂ and 1.7 mol of H₂. The following reaction becomes possible: CO(g) +H₂O(g) CO₂ (g) + H₂(g) The equilibrium constant K for this reaction is 9.79 at the temperature of the flask. Calculate the equilibrium molarity of CO₂. Round your answer to two decimal places. M X S

Suppose a 250. mL flask is filled with 0.80 mol of H₂O, 0.50 mol of CO₂ and 1.7 mol of H₂. The following reaction becomes possible: CO(g) +H₂O(g) CO₂ (g) + H₂(g) The equilibrium constant K for this reaction is 9.79 at the temperature of the flask. Calculate the equilibrium molarity of CO₂. Round your answer to two decimal places. M X S

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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4.
= O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 250. mL flask is filled with 1.3 mol of H₂ and 1.2 mol of HI. The following reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) The equilibrium constant K for this reaction is 6.96 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. ☐M X 3