(D) The reaction is $A_{(g)} + B_{(g)} \rightleftharpoons 2C_{(g)}$.Initial moles: $A = 3$,$B = 1$,$C = 0$.At equilibrium,$1.5 \ mol$ of $C$ are forme

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(D) The reaction is $A_{(g)} + B_{(g)} \rightleftharpoons 2C_{(g)}$.Initial moles: $A = 3$,$B = 1$,$C = 0$.At equilibrium,$1.5 \ mol$ of $C$ are formed. Since the stoichiometry of $C$ is $2$,the moles of $A$ and $B$ reacted are $1.5 / 2 = 0.75 \ mol$ each.Equilibrium moles: $A = 3 - 0.75 = 2.25 \ mol$,$B = 1 - 0.75 = 0.25 \ mol$,$C = 1.5 \ mol$.Since the volume is $1 \ L$,the concentrations are equal to the number of moles.$K_c = \frac{[C]^2}{[A][B]} = \frac{(1.5)^2}{(2.25)(0.25)} = \frac{2.25}{0.5625} = 4$.

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Kp and Kc Relationship

Medium

When $3 \ mol$ of $A$ and $1 \ mol$ of $B$ are mixed in a $1 \ L$ vessel,the following reaction takes place: $A_{(g)} + B_{(g)} \rightleftharpoons 2C_{(g)}$. If $1.5 \ mol$ of $C$ are formed at equilibrium,the equilibrium constant $(K_c)$ for the reaction is:

A
$0.12$
B
$0.25$
C
$0.5$
D
$4$

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Class 11 Questions

Class 11

Chemistry Questions

Chapter

1 Equilibrium: Chemical Equilibrium

Subtopic

Kp and Kc Relationship

Explain why the partial pressure $p$ of a gas is proportional to its concentration $c$.

Medium

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At $1000 \, K$,for the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)}$,the value of $K_p$ is $0.05 \, atm$. What will be the value of $K_c$ in terms of $R$?

Medium

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At $1000 \ K$,the value of $K_c$ for the reaction $A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)}$ is $10 \ mol \ L^{-1}$. The value of $K_p$ (in $atm$) is: (Given $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$)

EasyAP EAMCET 2023

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For the reaction $AB_{(g)} \rightleftharpoons A_{(g)} + B_{(g)}$,$AB$ is $33.3\%$ dissociated at a total equilibrium pressure of $P$. Therefore,$P$ is correctly related to $K_p$ by which of the following options?

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For a given exothermic reaction,$K_p$ and $K'_p$ are the equilibrium constants at temperatures $T_1$ and $T_2,$ respectively. Assuming that the heat of reaction is constant in the temperature range between $T_1$ and $T_2,$ where $T_2 > T_1,$ it is readily observed that:

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When $3 \ mol$ of $A$ and $1 \ mol$ of $B$ are mixed in a $1 \ L$ vessel,the following reaction takes place: $A_{(g)} + B_{(g)} \rightleftharpoons 2C_{(g)}$. If $1.5 \ mol$ of $C$ are formed at equilibrium,the equilibrium constant $(K_c)$ for the reaction is:

Similar Questions

Explain why the partial pressure $p$ of a gas is proportional to its concentration $c$.

At $1000 \, K$,for the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)}$,the value of $K_p$ is $0.05 \, atm$. What will be the value of $K_c$ in terms of $R$?

At $1000 \ K$,the value of $K_c$ for the reaction $A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)}$ is $10 \ mol \ L^{-1}$. The value of $K_p$ (in $atm$) is: (Given $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$)

For the reaction $AB_{(g)} \rightleftharpoons A_{(g)} + B_{(g)}$,$AB$ is $33.3\%$ dissociated at a total equilibrium pressure of $P$. Therefore,$P$ is correctly related to $K_p$ by which of the following options?

For a given exothermic reaction,$K_p$ and $K'_p$ are the equilibrium constants at temperatures $T_1$ and $T_2,$ respectively. Assuming that the heat of reaction is constant in the temperature range between $T_1$ and $T_2,$ where $T_2 > T_1,$ it is readily observed that:

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