Refer to the Integrative Example. A gaseous mixture is prepared containing 0.100 mol each of CH₄(g), H₂O(g), CO₂(g), and H₂(g) in a 5.00 L flask. Then the mixture is allowed to come to equilibrium at 1000 K. What will be the equilibrium amount, in moles, of each gas?

Integrative Example

In the manufacture of ammonia, the chief source of hydrogen gas is the following reaction for the reforming of methane at high temperatures.

The following data are also given.

At 1000 K, 1.00 mol each of CH₄ and H₂O are allowed to come to equilibrium in a 10.0 L vessel. Calculate the number of moles of H₂ present at equilibrium. Would the yield of H₂ increase if the temperature were raised above 1000 K?

Transcribed Image Text:

CH4(g) + 2 H₂O(g) CO₂(g) + 4H₂(g) (15.20)