Chemistry

Chemistry

Problem

Consider the equilibrium 2SO2(g)+O2(g)⇌2SO3(g)2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g) at a temperature where Kp=3.0K_p = 3.0. A sealed container initially at equilibrium is disturbed so that the partial pressures become PSO2=1.5 atmP_{\text{SO}_2}=1.5\,\text{atm}, PO2=0.50 atmP_{\text{O}_2}=0.50\,\text{atm}, and PSO3=2.0 atmP_{\text{SO}_3}=2.0\,\text{atm}. What will be the net direction of the reaction as the system re-establishes equilibrium? a) No net change will occur because the disturbance does not affect QpQ_p. b) It will shift toward products because the calculated QpQ_p exceeds KpK_p. c) It will shift toward reactants because the calculated QpQ_p exceeds KpK_p. d) It will shift toward products because the calculated QpQ_p is less than KpK_p.
Intuitive explanation

The key is to calculate the reaction quotient QpQ_p using the current partial pressures, then compare it to KpK_p to predict which way the system must shift. If Qp<KpQ_p < K_p, the reaction shifts forward (toward products); if Qp>KpQ_p > K_p, it shifts backward (toward reactants). This tells you whether the system has too many reactants or too many products relative to equilibrium.

Intuitive explanation

The key is to calculate the reaction quotient QpQ_p using the current partial pressures, then compare it to KpK_p to predict which way the system must shift. If Qp<KpQ_p < K_p, the reaction shifts forward (toward products); if Qp>KpQ_p > K_p, it shifts backward (toward reactants). This tells you whether the system has too many reactants or too many products relative to equilibrium.

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