(C) For the first equilibrium: $SO_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons SO_{3(g)}$,the equilibrium constant is $K_1 = \frac{[SO_3]}{[SO_2][

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(C) For the first equilibrium: $SO_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons SO_{3(g)}$,the equilibrium constant is $K_1 = \frac{[SO_3]}{[SO_2][O_2]^{1/2}}$.For the second equilibrium: $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$,the equilibrium constant is $K_2 = \frac{[SO_2]^2 [O_2]}{[SO_3]^2}$.Comparing the two expressions,we see that $K_2 = \left( \frac{1}{K_1} \right)^2 = \frac{1}{K_1^2}$.Therefore,the correct relationship is $K_2 = \frac{1}{K_1^2}$.

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

Medium

Two gaseous equilibria $SO_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons SO_{3(g)}$ and $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$ have equilibrium constants $K_1$ and $K_2$ respectively at $298 \ K$. Which of the following relationships between $K_1$ and $K_2$ is correct?

AIPMT 1989 All AIPMT

A
$K_1 = K_2$
B
$K_2 = K_1^2$
C
$K_2 = \frac{1}{K_1^2}$
D
$K_2 = \frac{1}{K_1}$

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Class 11

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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AIPMT 1989 Paper All AIPMT years →

For the reversible reaction, $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$. When the partial pressure is measured in atmosphere, the value of $K_p$ at $500^{\circ}\text{C}$ is $1.44 \times 10^{-5}$. The value of $K_c$ when the concentration is expressed in $\text{mol L}^{-1}$ is:

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The equilibrium constant for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ at temperature $T$ is $4 \times 10^{-4}$. The value of $K_c$ for the reaction $NO_{(g)} \rightleftharpoons \frac{1}{2}N_{2(g)} + \frac{1}{2}O_{2(g)}$ at the same temperature is

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For the following three equilibria $X, Y$,and $Z$ in the gaseous state at $300 \ K$,the increasing order of the ratio of $K_p$ to $K_c$ is:
$X: 2SO_2 + O_2 \rightleftharpoons 2SO_3$
$Y: PCl_5 \rightleftharpoons PCl_3 + Cl_2$
$Z: 2HI \rightleftharpoons H_2 + I_2$

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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For the decomposition reaction $N_2O_4 \rightleftharpoons 2NO_2$ at constant temperature,the equilibrium constant is given by $K_p = \frac{4x^2P}{1 - x^2}$,where $P$ is the total pressure and $x$ is the degree of dissociation. Which of the following statements is correct?

Medium

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Two gaseous equilibria $SO_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons SO_{3(g)}$ and $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$ have equilibrium constants $K_1$ and $K_2$ respectively at $298 \ K$. Which of the following relationships between $K_1$ and $K_2$ is correct?

Similar Questions

For the reversible reaction, $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$. When the partial pressure is measured in atmosphere, the value of $K_p$ at $500^{\circ}\text{C}$ is $1.44 \times 10^{-5}$. The value of $K_c$ when the concentration is expressed in $\text{mol L}^{-1}$ is:

The equilibrium constant for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ at temperature $T$ is $4 \times 10^{-4}$. The value of $K_c$ for the reaction $NO_{(g)} \rightleftharpoons \frac{1}{2}N_{2(g)} + \frac{1}{2}O_{2(g)}$ at the same temperature is

For the following three equilibria $X, Y$,and $Z$ in the gaseous state at $300 \ K$,the increasing order of the ratio of $K_p$ to $K_c$ is:$X: 2SO_2 + O_2 \rightleftharpoons 2SO_3$$Y: PCl_5 \rightleftharpoons PCl_3 + Cl_2$$Z: 2HI \rightleftharpoons H_2 + I_2$

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 $(R = 0.082 \ L \ bar \ mol^{-1} \ K^{-1})$.

For the decomposition reaction $N_2O_4 \rightleftharpoons 2NO_2$ at constant temperature,the equilibrium constant is given by $K_p = \frac{4x^2P}{1 - x^2}$,where $P$ is the total pressure and $x$ is the degree of dissociation. Which of the following statements is correct?

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For the following three equilibria $X, Y$,and $Z$ in the gaseous state at $300 \ K$,the increasing order of the ratio of $K_p$ to $K_c$ is:
$X: 2SO_2 + O_2 \rightleftharpoons 2SO_3$
$Y: PCl_5 \rightleftharpoons PCl_3 + Cl_2$
$Z: 2HI \rightleftharpoons H_2 + I_2$