(C) The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n_g}$.For $K_p = K_c$,the change in the number of moles of gaseous pro

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$H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$

(C) The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n_g}$.For $K_p = K_c$,the change in the number of moles of gaseous products and reactants must be zero,i.e.,$\Delta n_g = 0$.In option $(C)$,the reaction is $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$.Here,$\Delta n_g = (2) - (1 + 1) = 0$.Therefore,$K_p = K_c$ for this reaction.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Kp and Kc Relationship

Medium

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

A
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$
B
$2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2(g)}$
C
$H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$
D
$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

The equilibrium constant of $NH_4COONH_2$ in a closed vessel at $400 \ K$ temperature is $600 \ bar^3$. What will be the total pressure at equilibrium (in $bar$)?
$NH_4COONH_{2(s)} \rightleftharpoons 2NH_{3(g)} + CO_{2(g)}$

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For the reaction ${N_{2(g)}} + {O_{2(g)}} \rightleftharpoons 2NO_{(g)}$,the value of $K_c$ at $400 \ K$ is $4.0 \times 10^{-6}$. The value of $K_p$ for this reaction is .....

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In which of the following equilibria,$K_p$ and $K_c$ are $NOT$ equal?

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For a reversible reaction $A \rightleftharpoons B$,the equilibrium concentration of $B$,denoted as $[B]_e$,is given by which expression?

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For the reaction $2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2(g)}$,the value of equilibrium constant $K_p$ is $0.033 \ bar$ at $1060 \ K$. Calculate the value of $K_c$.

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

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The equilibrium constant of $NH_4COONH_2$ in a closed vessel at $400 \ K$ temperature is $600 \ bar^3$. What will be the total pressure at equilibrium (in $bar$)?$NH_4COONH_{2(s)} \rightleftharpoons 2NH_{3(g)} + CO_{2(g)}$

For the reaction ${N_{2(g)}} + {O_{2(g)}} \rightleftharpoons 2NO_{(g)}$,the value of $K_c$ at $400 \ K$ is $4.0 \times 10^{-6}$. The value of $K_p$ for this reaction is .....

In which of the following equilibria,$K_p$ and $K_c$ are $NOT$ equal?

For a reversible reaction $A \rightleftharpoons B$,the equilibrium concentration of $B$,denoted as $[B]_e$,is given by which expression?

For the reaction $2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2(g)}$,the value of equilibrium constant $K_p$ is $0.033 \ bar$ at $1060 \ K$. Calculate the value of $K_c$.

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The equilibrium constant of $NH_4COONH_2$ in a closed vessel at $400 \ K$ temperature is $600 \ bar^3$. What will be the total pressure at equilibrium (in $bar$)?
$NH_4COONH_{2(s)} \rightleftharpoons 2NH_{3(g)} + CO_{2(g)}$