The value of K_p for the following reaction 2 | vedclass

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(B) The relationship between $K_p$ and $K_c$ is given by the equation $K_p = K_c(RT)^{\Delta n}$.For the reaction $2H_2S_{(g)} \rightleftharpoons 2H_{

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$< 1.2 	imes 10^{-2}$

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(B) The relationship between $K_p$ and $K_c$ is given by the equation $K_p = K_c(RT)^{\Delta n}$.For the reaction $2H_2S_{(g)} ightleftharpoons 2H_{2(g)} + S_{2(g)}$,the change in the number of moles of gaseous products and reactants is $\Delta n = (2 + 1) - 2 = 1$.Substituting $\Delta n = 1$ into the equation,we get $K_p = K_c(RT)^1$,which implies $K_c = K_p / (RT)$.Since the temperature $T = 106.5 + 273.15 = 379.65  K$ is greater than $1$,the value of $(RT)$ is much greater than $1$.Therefore,$K_c = K_p / (RT)$ will be less than $K_p$.Thus,$K_c < 1.2 	imes 10^{-2}$.

The value of $K_p$ for the following reaction $2H_2S_{(g)} \rightleftharpoons 2H_{2(g)} + S_{2(g)}$ is $1.2 \times 10^{-2}$ at $106.5 ^oC$. The value of $K_c$ for this reaction is

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