Concerning the reaction in Exercise 26 and the situation described in part (c) of that exercise, will the mole fraction of C₂H₂(g) increase, decrease, or remain unchanged when equilibrium is re-established? Explain.

Exercise 26

At 2000 K, K_c = 0.154 for the reaction 2 CH₄(g) ⇌ C₂H₂(g) + 3 H₂(g). If a 1.00 L equilibrium mixture at 2000 K contains 0.10 mol each of CH₄(g) and H₂(g), 

(a) What is the mole fraction of C₂H₂(g) present?

(b) Is the conversion of CH₄(g) to C₂H₂(g) favored at high or low pressures?

(c) If the equilibrium mixture at 2000 K is transferred from a 1.00 L flask to a 2.00 L flask, will the number of moles of C₂H₂(g) increase, decrease, or remain unchanged?