(B) The relationship between $K_P$ and $K_C$ is given by $K_P = K_C(RT)^{\Delta n_g}$,where $\Delta n_g$ is the change in the number of moles of gaseo

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$2C_{(s)} + O_{2(g)} \rightleftharpoons 2CO_{(g)}$

(B) The relationship between $K_P$ and $K_C$ is given by $K_P = K_C(RT)^{\Delta n_g}$,where $\Delta n_g$ is the change in the number of moles of gaseous products and reactants. $K_P$ and $K_C$ are different when $\Delta n_g \neq 0$. For option $B$: $2C_{(s)} + O_{2(g)} \rightleftharpoons 2CO_{(g)}$,$\Delta n_g = 2 - 1 = 1$. Since $\Delta n_g = 1 \neq 0$,$K_P$ and $K_C$ are different for this reaction.

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

Difficult

For which of the following equilibria are $K_P$ and $K_C$ different?

A
$N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$
B
$2C_{(s)} + O_{2(g)} \rightleftharpoons 2CO_{(g)}$
C
$PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$
D
$H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

For the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)}$,the value of $K_p$ at $1000 \ K$ is $0.05 \ atm$. The value of $K_c$ in terms of $R$ will be:

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For the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$,if the total pressure in the reaction vessel at $105 \ ^\circ C$ is $1.12 \ atm$,then the $K_p$ for this equilibrium will be .........

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$1 \ mol$ $N_2$ and $3 \ mol$ $H_2$ are heated at $473 \ K$ and $100 \ atm$ pressure. At equilibrium,the number of moles of $NH_3$ is $0.5 \ mol$. Calculate the equilibrium constant $K_p$ of the given reaction: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

Medium

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For the reaction $C_{(s)} + CO_{2(g)} \rightleftharpoons 2CO_{(g)}$,the partial pressures of $CO_2$ and $CO$ are $2.0 \ atm$ and $4.0 \ atm$ respectively. The value of $K_p$ for the reaction is ............ .

Medium

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In a $500 \,mL$ flask,the degree of dissociation of $PCl_5$ at equilibrium is $40 \%$ and the initial amount is $5 \,moles$. The value of equilibrium constant in $mol \,L^{-1}$ for the decomposition of $PCl_5$ is

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For which of the following equilibria are $K_P$ and $K_C$ different?

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For the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)}$,the value of $K_p$ at $1000 \ K$ is $0.05 \ atm$. The value of $K_c$ in terms of $R$ will be:

For the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$,if the total pressure in the reaction vessel at $105 \ ^\circ C$ is $1.12 \ atm$,then the $K_p$ for this equilibrium will be .........

$1 \ mol$ $N_2$ and $3 \ mol$ $H_2$ are heated at $473 \ K$ and $100 \ atm$ pressure. At equilibrium,the number of moles of $NH_3$ is $0.5 \ mol$. Calculate the equilibrium constant $K_p$ of the given reaction: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

For the reaction $C_{(s)} + CO_{2(g)} \rightleftharpoons 2CO_{(g)}$,the partial pressures of $CO_2$ and $CO$ are $2.0 \ atm$ and $4.0 \ atm$ respectively. The value of $K_p$ for the reaction is ............ .

In a $500 \,mL$ flask,the degree of dissociation of $PCl_5$ at equilibrium is $40 \%$ and the initial amount is $5 \,moles$. The value of equilibrium constant in $mol \,L^{-1}$ for the decomposition of $PCl_5$ is

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