For the following three equilibria X, Y,and Z | vedclass

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(C) The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n_g}$,which implies $\frac{K_p}{K_c} = (RT)^{\Delta n_g}$.Since $RT =

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$X < Z < Y$

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(C) The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n_g}$,which implies $\frac{K_p}{K_c} = (RT)^{\Delta n_g}$.Since $RT = 300R$ is constant and greater than $1$,the ratio $\frac{K_p}{K_c}$ increases as $\Delta n_g$ increases.Calculate $\Delta n_g$ (moles of gaseous products - moles of gaseous reactants) for each:For $X: \Delta n_g = 2 - (2 + 1) = -1$For $Y: \Delta n_g = (1 + 1) - 1 = 1$For $Z: \Delta n_g = (1 + 1) - 2 = 0$Comparing the values of $\Delta n_g$: $-1 Therefore,the increasing order of the ratio is $X < Z < Y$.

For the following three equilibria $X, Y$,and $Z$ in the gaseous state at $300 \ K$,the increasing order of the ratio of $K_p$ to $K_c$ is:
$X: 2SO_2 + O_2 \rightleftharpoons 2SO_3$
$Y: PCl_5 \rightleftharpoons PCl_3 + Cl_2$
$Z: 2HI \rightleftharpoons H_2 + I_2$

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For the following three equilibria $X, Y$,and $Z$ in the gaseous state at $300 \ K$,the increasing order of the ratio of $K_p$ to $K_c$ is:$X: 2SO_2 + O_2 \rightleftharpoons 2SO_3$$Y: PCl_5 \rightleftharpoons PCl_3 + Cl_2$$Z: 2HI \rightleftharpoons H_2 + I_2$