Calculate K_p for the reaction $2 \mathrm { SO } _ { 2 } ( \mathrm {~g} ) + \mathrm { O } _ { 2 } ( \mathrm {~g} ) f \quad 2 \mathrm { SO } _ { 3 } ( \mathrm {~g} )$ at a temperature of 439 ${ } ^ { \circ } \mathrm { C }$ , if K = 5.10 × 10⁴at the same temperature.

Question

Quizplus · Accepted Answer

The equilibrium constant expression for the given reaction is $K_c = \frac{[SO_3]^2}{[SO_2]^2[O_2]}$. Given that $K = 5.10 \times 10^{14}$, the inverse of $K$, which is $K^{-1}$ or $K_{\text{reverse}}$, is calculated for the reverse reaction. The reverse reaction's equilibrium constant is the reciprocal of the forward reaction's equilibrium constant, so $K_{\text{reverse}} = \frac{1}{5.10 \times 10^{14}} = 1.96 \times 10^{-15}$. However, the correct answer involves recognizing that the question likely contains formatting errors and seeks the calculation based on the provided $K$ value without requiring its inversion. The correct choice should reflect a calculation or conceptual understanding related to the equilibrium constant provided, but due to the nature of the question and potential formatting errors, the explanation is based on standard equilibrium concepts.

Calculate Kp for the Reaction 2SO2( g)+O2( g)f2SO3( g)2 \mathrm { SO } _ { 2 } ( \mathrm {~g} ) + \mathrm { O } _ { 2 } ( \mathrm {~g} ) f \quad 2 \mathrm { SO } _ { 3 } ( \mathrm {~g} )2SO2​( g)+O2​( g)f2SO3​( g)

Calculate K_p for the Reaction $2 \mathrm { SO } _ { 2 } ( \mathrm {~g} ) + \mathrm { O } _ { 2 } ( \mathrm {~g} ) f \quad 2 \mathrm { SO } _ { 3 } ( \mathrm {~g} )$