(D) The equilibrium constant $(K_c)$ is defined as the ratio of the rate constant of the forward reaction $(K_f)$ to the rate constant of the backward

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(D) The equilibrium constant $(K_c)$ is defined as the ratio of the rate constant of the forward reaction $(K_f)$ to the rate constant of the backward reaction $(K_b)$.Given: $K_f = 1.1 \times 10^{-2} \text{ min}^{-1}$ and $K_b = 1.5 \times 10^{-3} \text{ min}^{-1}$.$K_c = \frac{K_f}{K_b} = \frac{1.1 \times 10^{-2}}{1.5 \times 10^{-3}} = \frac{11 \times 10^{-3}}{1.5 \times 10^{-3}} = \frac{11}{1.5} = 7.33$.Therefore,the correct option is $(D)$.

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

Medium

The rate constant for forward and backward reactions of hydrolysis of ester are $1.1 \times 10^{-2} \text{ min}^{-1}$ and $1.5 \times 10^{-3} \text{ min}^{-1}$ respectively. The equilibrium constant for the reaction $CH_3COOC_2H_5 + H_2O \rightleftharpoons CH_3COOH + C_2H_5OH$ is: (in $.33$)

AIIMS 1999 All AIIMS

A
$4$
B
$5$
C
$6$
D
$7$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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AIIMS 1999 Paper All AIIMS years →

For the reaction ${H_2}_{(g)} + {I_2}_{(g)} \rightleftharpoons 2HI_{(g)}$ at $721 \ K$,the value of the equilibrium constant $({K_c})$ is $50$. When the equilibrium concentration of both is $0.5 \ M$,the value of ${K_p}$ under the same conditions will be:

MediumAIPMT 1990

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Consider the partial decomposition of $A$ as:
$2A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$
At equilibrium,a $700 \ mL$ gaseous mixture contains $100 \ mL$ of gas $C$ at $10 \ atm$ and $300 \ K$. What is the value of $K_P$ for the reaction?

Medium

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$K_{p} = 0.04 \ atm$ at $899 \ K$ for the equilibrium shown below. What is the equilibrium pressure of $C_{2}H_{6}$ when it is placed in a flask at $4.0 \ atm$ pressure and allowed to come to equilibrium?
$C_{2}H_{6(g)} \longleftrightarrow C_{2}H_{4(g)} + H_{2(g)}$

Medium

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For the reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,the value of $K_p$ at $800 \ ^oC$ is $1.16 \ atm$. If $1 \ mol$ of $CaCO_{3(s)}$ is taken in a $1 \ L$ container to start the reaction,what will be the partial pressure of $CO_2$ at equilibrium in $atm$?

Medium

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$2 \ mol$ $PCl_5$ is heated in a $4 \ L$ closed vessel at a definite temperature. At equilibrium,$55\%$ of $PCl_5$ remains undissociated. Find $K_c$. Reaction: $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$

Medium

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The rate constant for forward and backward reactions of hydrolysis of ester are $1.1 \times 10^{-2} \text{ min}^{-1}$ and $1.5 \times 10^{-3} \text{ min}^{-1}$ respectively. The equilibrium constant for the reaction $CH_3COOC_2H_5 + H_2O \rightleftharpoons CH_3COOH + C_2H_5OH$ is: (in $.33$)

Similar Questions

For the reaction ${H_2}_{(g)} + {I_2}_{(g)} \rightleftharpoons 2HI_{(g)}$ at $721 \ K$,the value of the equilibrium constant $({K_c})$ is $50$. When the equilibrium concentration of both is $0.5 \ M$,the value of ${K_p}$ under the same conditions will be:

Consider the partial decomposition of $A$ as:$2A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$At equilibrium,a $700 \ mL$ gaseous mixture contains $100 \ mL$ of gas $C$ at $10 \ atm$ and $300 \ K$. What is the value of $K_P$ for the reaction?

$K_{p} = 0.04 \ atm$ at $899 \ K$ for the equilibrium shown below. What is the equilibrium pressure of $C_{2}H_{6}$ when it is placed in a flask at $4.0 \ atm$ pressure and allowed to come to equilibrium?$C_{2}H_{6(g)} \longleftrightarrow C_{2}H_{4(g)} + H_{2(g)}$

For the reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,the value of $K_p$ at $800 \ ^oC$ is $1.16 \ atm$. If $1 \ mol$ of $CaCO_{3(s)}$ is taken in a $1 \ L$ container to start the reaction,what will be the partial pressure of $CO_2$ at equilibrium in $atm$?

$2 \ mol$ $PCl_5$ is heated in a $4 \ L$ closed vessel at a definite temperature. At equilibrium,$55\%$ of $PCl_5$ remains undissociated. Find $K_c$. Reaction: $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$

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Consider the partial decomposition of $A$ as:
$2A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$
At equilibrium,a $700 \ mL$ gaseous mixture contains $100 \ mL$ of gas $C$ at $10 \ atm$ and $300 \ K$. What is the value of $K_P$ for the reaction?

$K_{p} = 0.04 \ atm$ at $899 \ K$ for the equilibrium shown below. What is the equilibrium pressure of $C_{2}H_{6}$ when it is placed in a flask at $4.0 \ atm$ pressure and allowed to come to equilibrium?
$C_{2}H_{6(g)} \longleftrightarrow C_{2}H_{4(g)} + H_{2(g)}$