For the gas-phase reaction at 1000 K

CHEMISTRY · Single correct · A Level · Chemistry · Chemical equilibria (Le Chatelier’s principle and Kc) · Chemical equilibria (Le Chatelier’s principle and Kc)

Problem

For the gas-phase reaction 2 SO2(g)+O2(g)⇌2 SO3(g)2\,\text{SO}_2(g)+\text{O}_2(g)\rightleftharpoons 2\,\text{SO}_3(g) at 1000 K, the equilibrium constant is Kc=4.0K_c = 4.0. A mixture is prepared with [SO2]=0.15 M[\text{SO}_2]=0.15\,\text{M}, [O2]=0.050 M[\text{O}_2]=0.050\,\text{M}, and [SO3]=0.30 M[\text{SO}_3]=0.30\,\text{M}. Which of the following best describes how the concentrations will change as the system moves toward equilibrium? (a) [SO3][\text{SO}_3] will increase, while [SO2][\text{SO}_2] and [O2][\text{O}_2] will decrease. (b) All concentrations are already at equilibrium, so no net change will occur. (c) [SO3][\text{SO}_3] will decrease, while [SO2][\text{SO}_2] and [O2][\text{O}_2] will increase. (d) [SO2][\text{SO}_2] will decrease, while [SO3][\text{SO}_3] and [O2][\text{O}_2] will increase.

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