Consider the hypothetical reaction A(g) + 2B(g) = 2C(g), for which Kc = 0.25 at some temperature. A 1.00 L reaction vessel is loaded with 1.00 mol of compound C, which is allowed to reach equilibrium. Let the variable x represent the number of m/L of compound A present at equilibrium.

a) In terms of x, what are the equilibrium concentration of compound B and C?

b) What limits must be placed on the value of x so that all concentrations are positive?

c) By putting the equilibrium concentrations (in terms of x) into the equilibrium-constant expression, derive an equation that can be solved for x.