For the reaction 2SO_{2(g)} + O_{2(g)} rightl | vedclass

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Question

(C) For the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$,the change in the number of moles of gaseous products and reactants is $\De

Vedclass · Accepted Answer

$K_c - K_p = 	ext{positive}$

Vedclass · Answer

(C) For the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$,the change in the number of moles of gaseous products and reactants is $\Delta n_g = 2 - (2 + 1) = -1$.The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n_g}$.Substituting $\Delta n_g = -1$,we get $K_p = K_c(RT)^{-1} = \frac{K_c}{RT}$.Since $RT$ is typically greater than $1$ at standard temperatures,$K_c > K_p$,which implies $K_p - K_c$ is negative.However,looking at the options provided,the relationship $K_p = K_c(RT)^{-1}$ indicates that $K_p$ and $K_c$ are not equal. Given the options,$K_p - K_c$ is negative,which is not explicitly listed as a positive value. Re-evaluating the options,if $K_c > K_p$,then $K_c - K_p$ is positive.

For the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$,which of the following equations is correct?

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