(B) The given reaction is $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$.The relationship between $K_p$ and $K_c$ is given by the formula $K_p = K

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(B) The given reaction is $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$.The relationship between $K_p$ and $K_c$ is given by the formula $K_p = K_c(RT)^{\Delta n}$.Here,$\Delta n$ is the change in the number of moles of gaseous products and reactants: $\Delta n = (n_{products}) - (n_{reactants}) = 2 - (1 + 1) = 0$.Since $\Delta n = 0$,the expression becomes $K_p = K_c(RT)^0 = K_c \times 1 = K_c$.Given that $K_c = 0.1$,therefore $K_p = 0.1$.

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

Medium

For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the value of $K_c$ at $800 \ ^oC$ is $0.1$. When the equilibrium concentrations of both the reactants are $0.5 \ M$,what is the value of $K_p$ at the same temperature?

A
$0.5$
B
$0.1$
C
$0.01$
D
$0.025$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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MediumAIPMT 2002

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For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the value of $K_c$ at $800 \ ^oC$ is $0.1$. When the equilibrium concentrations of both the reactants are $0.5 \ M$,what is the value of $K_p$ at the same temperature?

Similar Questions

The equilibrium constant for the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$ is $K.$ Then,the equilibrium constant for the equilibrium $NH_3 \rightleftharpoons \frac{1}{2}N_2 + \frac{3}{2}H_2$ is

For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,the equilibrium constant $K_c = 1.8 \times 10^{-6}$ at $184 \, ^\circ C$. Comparing $K_p$ and $K_c$ at $184 \, ^\circ C$,we find that:

For the reaction $CO_{(g)} + Cl_{2(g)} \rightleftharpoons COCl_{2(g)}$,$\frac{K_p}{K_c}$ is equal to

For the following reaction in gaseous phase $CO + 1/2 O_2 \to CO_2$,the ratio $K_p/K_c$ is:

In which one of the following gaseous equilibria is $K_p$ less than $K_c$?

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