Consider the two gaseous equilibria: $\begin{array}{ll} \mathrm{SO}_{2}(\mathrm{g})+~^1/_2 \mathrm{O}_{2}(\mathrm{~g}) \leftrightharpoons \mathrm{SO}_{3}(\mathrm{g}) & \mathrm{K}_{1} \ 2 \mathrm{SO}_{3}(\mathrm{g}) \leftrightharpoons \mathrm{SO}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) & \mathrm{K}_{2} \end{array}$ The values of the equilibrium constants K₁ and K₂ are related by

Question

Quizplus · Accepted Answer

According to Le Chatelier's principle, when an equilibrium is disturbed, the reaction will proceed in a direction that opposes the change. In this case, if the equilibrium constant for reaction 1 (K₁) is increased by a factor of ², the equilibrium constant for reaction 2 (K₂) must decrease by the same factor in order to maintain equilibrium. Mathematically, this can be expressed as: K₂ = 1/(K₁*²) or equivalently K₂ = 1/K₁*². Therefore, the correct choice is C.

Consider the Two Gaseous Equilibria The Values of the Equilibrium Constants K1 and K2 Are

Consider the Two Gaseous Equilibria The Values of the Equilibrium Constants K₁ and K₂ Are