The reaction A(g) B(g) + C(g) was initiated with the amount 'a' of A(g). At equilibrium it is found that the amount of A(g) remaining is (a - x) at a total pressure of p. The equilibrium constant K_p of the reaction can be calculated from the expression :
B. x^2 a^2 - x^2 p
The reaction is A(g) B(g) + C(g) Initial moles: a for A, 0 for B, 0 for C Moles at equilibrium: (a - x) for A, x for B, x for C Total moles at equilibrium = (a - x) + x + x = a + x Partial pressures at equilibrium: p_A = a - x a + x p p_B = x a + x p p_C = x a + x p The equilibrium constant K_p is given by: K_p = p_B p_C p_A K_p = ( x a + x p ) ( x a + x p ) a - x a + x p K_p = x^2 (a + x)(a - x) p K_p = x^2 a^2 - x^2 p Answer: x^2 a^2 - x^2 p
Related: Chemistry — Chemical Equilibrium · All PYQ Banks