(C) The relationship between $K_p$ and $K_c$ is given by the equation: $K_p = K_c(RT)^{\Delta n_g}$.For $K_p = K_c$,the term $(RT)^{\Delta n_g}$ must

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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 the equation: $K_p = K_c(RT)^{\Delta n_g}$.For $K_p = K_c$,the term $(RT)^{\Delta n_g}$ must be equal to $1$,which implies $\Delta n_g = 0$.$\Delta n_g$ is the difference between the number of moles of gaseous products and gaseous reactants.For option $C$: $H_{2_{(g)}} + I_{2_{(g)}} \rightleftharpoons 2HI_{(g)}$,$\Delta n_g = 2 - (1 + 1) = 0$.Since $\Delta n_g = 0$,$K_p = K_c$ for this reaction.

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

Easy

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

A
$2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2_{(g)}}$
B
$N_{2_{(g)}} + 3H_{2_{(g)}} \rightleftharpoons 2NH_{3_{(g)}}$
C
$H_{2_{(g)}} + I_{2_{(g)}} \rightleftharpoons 2HI_{(g)}$
D
$2SO_{2_{(g)}} + O_{2_{(g)}} \rightleftharpoons 2SO_{3_{(g)}}$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

$A$ vessel at $1000 \ K$ contains $CO_2$ with a pressure of $0.5 \ atm$. Some of the $CO_2$ is converted into $CO$ on the addition of graphite. If the total pressure at equilibrium is $0.8 \ atm$,the value of $K_p$ is $..... \ atm$.

MediumAIEEE 2011

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For the reaction in equilibrium
$2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$
if $P_{Br_2}$ is $\frac{P}{9}$ at equilibrium and $P$ is the total pressure,then calculate $\frac{P}{K_P}$.

Medium

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For the formation of $NH_3$ from $N_2$ and $H_2$ at $500 \ K$,the concentrations of $N_2, H_2$ and $NH_3$ at equilibrium are $1.5 \times 10^{-2} \ M, 3.0 \times 10^{-2} \ M$ and $1.2 \times 10^{-2} \ M$,respectively. The equilibrium constant for the reverse reaction is

MediumTS EAMCET 2018

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For the reaction $CO_{(g)} + 2H_{2(g)} \rightleftharpoons CH_3OH_{(g)}$,the true condition is:

Medium

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For which of the following reactions will ${K_p} > {K_c}$?

Medium

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

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$A$ vessel at $1000 \ K$ contains $CO_2$ with a pressure of $0.5 \ atm$. Some of the $CO_2$ is converted into $CO$ on the addition of graphite. If the total pressure at equilibrium is $0.8 \ atm$,the value of $K_p$ is $..... \ atm$.

For the reaction in equilibrium$2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$if $P_{Br_2}$ is $\frac{P}{9}$ at equilibrium and $P$ is the total pressure,then calculate $\frac{P}{K_P}$.

For the formation of $NH_3$ from $N_2$ and $H_2$ at $500 \ K$,the concentrations of $N_2, H_2$ and $NH_3$ at equilibrium are $1.5 \times 10^{-2} \ M, 3.0 \times 10^{-2} \ M$ and $1.2 \times 10^{-2} \ M$,respectively. The equilibrium constant for the reverse reaction is

For the reaction $CO_{(g)} + 2H_{2(g)} \rightleftharpoons CH_3OH_{(g)}$,the true condition is:

For which of the following reactions will ${K_p} > {K_c}$?

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For the reaction in equilibrium
$2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$
if $P_{Br_2}$ is $\frac{P}{9}$ at equilibrium and $P$ is the total pressure,then calculate $\frac{P}{K_P}$.