(A) The relationship between $K_p$ and $K_c$ is given by the equation: $K_p = K_c(RT)^{\Delta n_g}$.For $K_p$ to be equal to $K_c$,the term $(RT)^{\De

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$H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$

(A) The relationship between $K_p$ and $K_c$ is given by the equation: $K_p = K_c(RT)^{\Delta n_g}$.For $K_p$ to be equal to $K_c$,the term $(RT)^{\Delta n_g}$ must be equal to $1$,which occurs when $\Delta n_g = 0$.$\Delta n_g$ is defined as the difference between the sum of stoichiometric coefficients of gaseous products and gaseous reactants: $\Delta n_g = \sum n_p - \sum n_r$.For option $A$: $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$,$\Delta n_g = 2 - (1 + 1) = 0$.Since $\Delta n_g = 0$,$K_p = K_c$ for this reaction.

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

Medium

In which of the following reactions is the value of $K_p$ equal to $K_c$?

A
$H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$
B
$PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$
C
$2NH_3(g) \rightleftharpoons N_2(g) + 3H_2(g)$
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

The half-life of forward and reverse reactions are $400 \, sec$ and $100 \, sec$ respectively. If these half-lives are independent of the concentration of the reactant,find the equilibrium constant of the reaction.

Medium

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In a system $A_{(s)} \rightleftharpoons 2B_{(g)} + 3C_{(g)},$ if the concentration of $C$ at equilibrium is increased by a factor of $2,$ it will cause the equilibrium concentration of $B$ to change to

Medium

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For a reaction $2A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$,$K_c = 3.75 \times 10^{-6}$ at $1069 \ K$. The approximate value of $K_p$ for this reaction at the same temperature is $(R = 0.082 \ L \ bar \ mol^{-1} \ K^{-1})$.

MediumTS EAMCET 2018

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At $400 \ K$,in a $1.0 \ L$ vessel,$N_2O_4$ is allowed to attain equilibrium,$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$. At equilibrium,the total pressure is $600 \ mm \ Hg$,when $20 \%$ of $N_2O_4$ is dissociated. The value of $K_p$ for the reaction is

DifficultAP EAMCET 2016

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$K_p$ for the reaction $2SO_3 \rightleftharpoons 2SO_2 + O_2$ at $700 \ K$ is $1.3 \times 10^{-3} \ atm$. The $K_c$ at the same temperature for the reaction $2SO_2 + O_2 \rightleftharpoons 2SO_3$ will be:

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In which of the following reactions is the value of $K_p$ equal to $K_c$?

Similar Questions

The half-life of forward and reverse reactions are $400 \, sec$ and $100 \, sec$ respectively. If these half-lives are independent of the concentration of the reactant,find the equilibrium constant of the reaction.

In a system $A_{(s)} \rightleftharpoons 2B_{(g)} + 3C_{(g)},$ if the concentration of $C$ at equilibrium is increased by a factor of $2,$ it will cause the equilibrium concentration of $B$ to change to

For a reaction $2A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$,$K_c = 3.75 \times 10^{-6}$ at $1069 \ K$. The approximate value of $K_p$ for this reaction at the same temperature is $(R = 0.082 \ L \ bar \ mol^{-1} \ K^{-1})$.

At $400 \ K$,in a $1.0 \ L$ vessel,$N_2O_4$ is allowed to attain equilibrium,$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$. At equilibrium,the total pressure is $600 \ mm \ Hg$,when $20 \%$ of $N_2O_4$ is dissociated. The value of $K_p$ for the reaction is

$K_p$ for the reaction $2SO_3 \rightleftharpoons 2SO_2 + O_2$ at $700 \ K$ is $1.3 \times 10^{-3} \ atm$. The $K_c$ at the same temperature for the reaction $2SO_2 + O_2 \rightleftharpoons 2SO_3$ will be:

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