A reaction vessel contains a mixture of gaseous H2, N2 and NH3 that is initially at equilibrium. The

A reaction vessel contains a mixture of gaseous H2, N2 and NH3 that is initially at equilibrium. The volume of the reaction vessel is doubled (while the temperature remains constant), which means that the partial pressures of H2, N2 and NH3 are halved. What effect does this have on the equilibrium constant, Kp for the reaction 𝑁2 (𝑔) + 3𝐻2 (𝑔) ⇌ 2𝑁𝐻3 (𝑔)?

A) The value of Kp doubles B) The value of Kp halves C) The value of Kp is increased by a factor of 4

D) The value of Kp is decreased by a factor of 4

E) There will be no change in Kp

Explanation: The value of equilibrium constant K (can be Kp or Kc) only changes with temperature. No other factors such as volume or concentrations will affect it.

Answer: E) There will be no change in Kp