Solid species A reacts with gas B to form gas C with the following stoichiometry:

At 500 K, the equilibrium constant for the reaction is K = 4. The system is held at a constant pressure of 3 bar and initially has 1 mole of B and plenty of solid A. You may assume ideal gas behavior.

(a) If the reaction proceeds to equilibrium, how many moles of C will form?

(b) For the same temperature, can you increase the equilibrium conversion by changing pressure?
If so, would you raise or lower P? Explain.

Transcribed Image Text:

A(s) + B(g) 2C(g)