8. Consider the reaction: CO + 3H2(g) ↔ CH4(g) + H2O(g) At 500 K, the equilibrium constant for this reaction is KP = 2.48 × 10^-3. Suppose we fill a 7.50 L flask with the four gases. When the mixture reaches equilibrium, the flask contains 0.521 g CO, 0.521 g H2, and 9.20 g H2O. How many grams of CH4 are present?
8. Consider the reaction: CO + 3H2(g) ↔ CH4(g) + H2O(g) At 500 K, the equilibrium constant for this reaction is KP = 2.48 × 10^-3. Suppose we fill a 7.50 L flask with the four gases. When the mixture reaches equilibrium, the flask contains 0.521 g CO, 0.521 g H2, and 9.20 g H2O. How many grams of CH4 are present?
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 13Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...
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8. Consider the reaction:
CO + 3H2(g) ↔ CH4(g) + H2O(g)
At 500 K, the equilibrium constant for this reaction is KP = 2.48 × 10^-3. Suppose we fill a 7.50 L flask with the four gases. When the mixture reaches equilibrium, the flask contains 0.521 g CO, 0.521 g H2, and 9.20 g H2O. How many grams of CH4 are present?
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