Value of K_{p} for the equilibrium reaction N | vedclass

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(A) The relationship between $K_{p}$ and $K_{c}$ is given by the formula: $K_{p} = K_{c}(RT)^{\Delta n_{g}}$.For the reaction $N_{2}O_{4(g)} \rightlef

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$2$

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(A) The relationship between $K_{p}$ and $K_{c}$ is given by the formula: $K_{p} = K_{c}(RT)^{\Delta n_{g}}$.For the reaction $N_{2}O_{4(g)} ightleftharpoons 2NO_{2(g)}$,the change in the number of moles of gaseous species is $\Delta n_{g} = 2 - 1 = 1$.Given $K_{p} = 47.9$,$R = 0.083 \ L \ 	ext{bar} \ K^{-1} \ mol^{-1}$,and $T = 288 \ K$.Substituting the values: $47.9 = K_{c} 	imes (0.083 	imes 288)^{1}$.$K_{c} = \frac{47.9}{0.083 	imes 288} = \frac{47.9}{23.904} \approx 2.0038$.Rounding to the nearest integer,we get $K_{c} = 2$.

Value of $K_{p}$ for the equilibrium reaction $N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)}$ at $288 \ K$ is $47.9$. The $K_{C}$ for this reaction at same temperature is $......$ (Nearest integer)
$(R=0.083 \ L \ \text{bar} \ K^{-1} \ mol^{-1})$

Similar Questions

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

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For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,$K_c = 1.8 \times 10^{-6}$ at $184 \, ^\circ C$. Given $R = 0.0831 \, kJ/(mol \cdot K)$,when $K_p$ and $K_c$ are compared at $184 \, ^\circ C$,it is found that:

In which of the following equilibrium $K_c$ and $K_p$ are not equal?

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Value of $K_{p}$ for the equilibrium reaction $N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)}$ at $288 \ K$ is $47.9$. The $K_{C}$ for this reaction at same temperature is $......$ (Nearest integer)$(R=0.083 \ L \ \text{bar} \ K^{-1} \ mol^{-1})$