Suppose a 250. mL flask is filled with 1.6 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible:(3)H+(3)0ɔ= (3)0°H+(3)0)The equilibrium constant K for this reaction is 0.735 at the temperature of the flask.Calculate the equilibrium molarity of CO. Round your answer to two decimal places.OM

Moles of CO = 1.6 molMoles of H2O = 2.0 molMoles of CO2 =0.9 molK = 0.735

Suppose a 250. mL flask is filled with 1.6 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible: Co (g) + H,O(g) – Co,g)+H,(g) The equilibrium constant K for this reaction is 0.735 the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.

Suppose a 250. mL flask is filled with 1.6 mol of CO, 2.0 mol of H,0 and 0.90 mol of CO,. The following reaction becomes possible: Co (g) + H,O(g) – Co,g)+H,(g) The equilibrium constant K for this reaction is 0.735 the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.

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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