Chemistry

Problem

Ammonia is formed according to

\text{N}_2\,(g) + 3\,\text{H}_2\,(g) \rightleftharpoons 2\,\text{NH}_3\,(g)

. At a certain temperature the equilibrium partial pressures in a sealed vessel are

P_{\text{N}_2}=0.80\,\text{atm}

P_{\text{H}_2}=2.4\,\text{atm}

, and

P_{\text{NH}_3}=0.80\,\text{atm}

. The volume of the vessel is then doubled instantaneously at the same temperature. Which statement correctly describes the relationship between the reaction quotient

Q_{\text p}

(immediately after the volume change) and the equilibrium constant

K_{\text p}

, and the direction in which the reaction will proceed? a)

Q_{\text p} < K_{\text p}

; the reaction will form more products. b)

Q_{\text p} = K_{\text p}

; the system remains at equilibrium. c)

Q_{\text p} > K_{\text p}

; the reaction will form more reactants. d)

Q_{\text p} > K_{\text p}

; the reaction will form more products.

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