Consider the gas-phase reaction, N 2 (g) + 3 H 2 (g) <=> 2 NH 3 (g), for which K
ID: 895526 • Letter: C
Question
Consider the gas-phase reaction, N2(g) + 3 H2(g) <=> 2 NH3 (g), for which Kp = 43 at 400 K. If the mixture is analyzed and found to contain 0.6 bar of N2, 0.4 bar of H2 and 1.4 bar of NH3, describe the situation
Q < K and more reactants will be made to reach equilibrium.
Q > K and more products will be made to reach equilibrium.
Within 1 decimal place, Q = K and the reaction is at equilibrium
Q > K and more reactants will be made to reach equilibrium.
Q < K and more products will be made to reach equilibrium.
1.Q < K and more reactants will be made to reach equilibrium.
2.Q > K and more products will be made to reach equilibrium.
3.Within 1 decimal place, Q = K and the reaction is at equilibrium
4.Q > K and more reactants will be made to reach equilibrium.
5.Q < K and more products will be made to reach equilibrium.
Explanation / Answer
N2(g) + 3 H2(g) <=> 2 NH3 (g)
Q = [NH3]2 / [N2][H2]3
Q = (1.4)^2 / (0.6)*(0.4)^3
Q = 51
so here Q> K so the reaction favors towards reactents side
so option 4 is correct