(C) The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n_g}$,which implies $\frac{K_p}{K_c} = (RT)^{\Delta n_g}$.Since $RT =

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(C) The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n_g}$,which implies $\frac{K_p}{K_c} = (RT)^{\Delta n_g}$.Since $RT = 300R$ is constant and greater than $1$,the ratio $\frac{K_p}{K_c}$ increases as $\Delta n_g$ increases.Calculate $\Delta n_g$ (moles of gaseous products - moles of gaseous reactants) for each:For $X: \Delta n_g = 2 - (2 + 1) = -1$For $Y: \Delta n_g = (1 + 1) - 1 = 1$For $Z: \Delta n_g = (1 + 1) - 2 = 0$Comparing the values of $\Delta n_g$: $-1 Therefore,the increasing order of the ratio is $X < Z < Y$.

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

Medium

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:
$X: 2SO_2 + O_2 \rightleftharpoons 2SO_3$
$Y: PCl_5 \rightleftharpoons PCl_3 + Cl_2$
$Z: 2HI \rightleftharpoons H_2 + I_2$

A
$X = Y = Z$
B
$X < Y < Z$
C
$X < Z < Y$
D
$Z < Y < X$

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Class 11

Chemistry Questions

Chapter

6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

For the reaction $H_2 + I_2 \rightleftharpoons 2HI$,the equilibrium concentrations of $H_2$,$I_2$,and $HI$ are $8.0 \ mol \ L^{-1}$,$3.0 \ mol \ L^{-1}$,and $28.0 \ mol \ L^{-1}$ respectively. The equilibrium constant $(K_c)$ of the reaction is: (in $.66$)

MediumAIPMT 2001

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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?

MediumAIPMT 1989

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In a chemical equilibrium,the rate constant of the backward reaction is $7.5 \times 10^{-4}$ and the equilibrium constant is $1.5$. The rate constant of the forward reaction is:

Medium

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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

EasyAIIMS 1999

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For the reaction $PCl_{3(g)} + Cl_{2(g)} \rightleftharpoons PCl_{5(g)}$,the value of $K_p$ at $250 \ ^oC$ is $0.61 \ atm^{-1}$. The value of $K_c$ at this temperature will be .... $(mol \ L^{-1})$.

Medium

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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$

Similar Questions

For the reaction $H_2 + I_2 \rightleftharpoons 2HI$,the equilibrium concentrations of $H_2$,$I_2$,and $HI$ are $8.0 \ mol \ L^{-1}$,$3.0 \ mol \ L^{-1}$,and $28.0 \ mol \ L^{-1}$ respectively. The equilibrium constant $(K_c)$ of the reaction is: (in $.66$)

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?

In a chemical equilibrium,the rate constant of the backward reaction is $7.5 \times 10^{-4}$ and the equilibrium constant is $1.5$. The rate constant of the forward reaction is:

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 $PCl_{3(g)} + Cl_{2(g)} \rightleftharpoons PCl_{5(g)}$,the value of $K_p$ at $250 \ ^oC$ is $0.61 \ atm^{-1}$. The value of $K_c$ at this temperature will be .... $(mol \ L^{-1})$.

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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:
$X: 2SO_2 + O_2 \rightleftharpoons 2SO_3$
$Y: PCl_5 \rightleftharpoons PCl_3 + Cl_2$
$Z: 2HI \rightleftharpoons H_2 + I_2$