Equilibrium constants K_1 and K_2 for the fol | vedclass

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Question

(D) For the first equilibrium: $NO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons NO_{2(g)}$,the equilibrium constant is $K_1 = \frac{[NO_2]}{[NO][O_2]^{1/2}

Vedclass · Accepted Answer

$K_2 = 1 / K_1^2$

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(D) For the first equilibrium: $NO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons NO_{2(g)}$,the equilibrium constant is $K_1 = \frac{[NO_2]}{[NO][O_2]^{1/2}}$.For the second equilibrium: $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,the equilibrium constant is $K_2 = \frac{[NO]^2[O_2]}{[NO_2]^2}$.Observe that the second reaction is the reverse of the first reaction multiplied by $2$.If a reaction is reversed,the equilibrium constant becomes $1/K$. If a reaction is multiplied by a factor $n$,the equilibrium constant becomes $K^n$.Here,the first reaction is reversed and multiplied by $2$,so $K_2 = (1/K_1)^2 = 1/K_1^2$.

Equilibrium constants $K_1$ and $K_2$ for the following equilibria are given:
$NO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons NO_{2(g)}$
$2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$
What is the relationship between $K_1$ and $K_2$?

Similar Questions

Given the equilibria:
$I: A + 2B \rightleftharpoons C ; K_{eq} = K_1$
$II: C + D \rightleftharpoons 3A ; K_{eq} = K_2$
$III: 6B + D \rightleftharpoons 2C ; K_{eq} = K_3$
Which of the following relations is correct?

Assertion : For reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the unit of $K_C$ is $L^2 \, mol^{-2}$.
Reason : For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the equilibrium constant $K_C = \frac{[NH_3]^2}{[N_2][H_2]^3}$.

The value of $K_p$ for the following reaction $2H_2S_{(g)} \rightleftharpoons 2H_{2(g)} + S_{2(g)}$ is $1.2 \times 10^{-2}$ at $106.5 ^oC$. The value of $K_c$ for this reaction is

For the reaction $NH_4COONH_2(s) \rightleftharpoons 2NH_3(g) + CO_2(g)$,the equilibrium pressure is $3 \ atm$. Calculate $K_p$.

One mole of $PCl_5$ is heated in a closed container of $1 \ L$ capacity. At equilibrium,$20\%$ of $PCl_5$ is not dissociated. What should be the value of $K_C$?

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Equilibrium constants $K_1$ and $K_2$ for the following equilibria are given:$NO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons NO_{2(g)}$$2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$What is the relationship between $K_1$ and $K_2$?