In which of the following reactions is {K_p} | vedclass

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(D) The relationship between ${K_p}$ and ${K_c}$ is given by the equation: ${K_p} = {K_c}{(RT)}^{\Delta n}$.For ${K_p} > {K_c}$,the value of $\Delta n

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$2S{O_3} \rightleftharpoons {O_2} + 2S{O_2}$

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(D) The relationship between ${K_p}$ and ${K_c}$ is given by the equation: ${K_p} = {K_c}{(RT)}^{\Delta n}$.For ${K_p} > {K_c}$,the value of $\Delta n$ must be positive $(\Delta n > 0)$.$\Delta n$ is calculated as the difference between the number of moles of gaseous products and gaseous reactants.$(A)$ ${N_2} + 3{H_2} \rightleftharpoons 2N{H_3}$: $\Delta n = 2 - (1 + 3) = -2$$(B)$ ${H_2} + {I_2} \rightleftharpoons 2HI$: $\Delta n = 2 - (1 + 1) = 0$$(C)$ $PC{l_3} + C{l_2} \rightleftharpoons PC{l_5}$: $\Delta n = 1 - (1 + 1) = -1$$(D)$ $2S{O_3} \rightleftharpoons {O_2} + 2S{O_2}$: $\Delta n = (1 + 2) - 2 = +1$Since $\Delta n = +1$ for reaction $(D)$,${K_p} > {K_c}$ holds true for this reaction.

In which of the following reactions is ${K_p} > {K_c}$?

Similar Questions

At $298 \ K$,the value of $K_c$ for the following reaction is $x \ mol \ L^{-1}$. What is the approximate $K_p$ value for this reaction? $(R=0.082 \ L \ atm \ mol^{-1} \ K^{-1})$ $A_2O_{4(g)} \rightleftharpoons 2AO_{2(g)}$

In which of the following cases is $K_p$ less than $K_c$?

In a chemical equilibrium,the rate constant of the backward reaction is $7.5 \times 10^{-4}$ and the equilibrium constant is $1.5$. The rate constant of the forward reaction is:

For which of the following reactions is $K_p = K_c$?

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