(C) The concentrations of the species are: $[A] = \frac{2 \ mol}{100 \ L} = 0.02 \ M$,$[B] = \frac{0.25 \ mol}{100 \ L} = 0.0025 \ M$,and $[C] = \frac

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(C) The concentrations of the species are: $[A] = \frac{2 \ mol}{100 \ L} = 0.02 \ M$,$[B] = \frac{0.25 \ mol}{100 \ L} = 0.0025 \ M$,and $[C] = \frac{0.5 \ mol}{100 \ L} = 0.005 \ M$. The reaction quotient $Q_c$ is calculated as: $Q_c = \frac{[C]^2}{[A]^2[B]} = \frac{(0.005)^2}{(0.02)^2 \times 0.0025} = \frac{0.000025}{0.0004 \times 0.0025} = \frac{0.000025}{0.000001} = 25$. Since $Q_c = K_c = 25$,the reaction is in a state of equilibrium.

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

Easy

Consider a reversible reaction $2A + B \rightleftharpoons 2C$ having equilibrium constant $K_c = 25$. If a reaction vessel contains $2 \ mol$ of $A$,$0.25 \ mol$ of $B$,and $0.5 \ mol$ of $C$ in a $100 \ L$ vessel,what will be the direction of the reaction?

A
Forward
B
Backward
C
Exist in equilibrium
D
Can't predict

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1 Equilibrium: Chemical Equilibrium

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Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

For the reaction $SO_{2(g)} + NO_{2(g)} \rightleftharpoons SO_{3(g)} + NO_{(g)}$,the equilibrium constant $K_c$ is $16$. If $1 \ mol$ of each gas is taken in a $1 \ dm^3$ vessel,the equilibrium concentration of $NO$ will be ....

Medium

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Consider the following chemical equilibrium of the gas phase reaction at a constant temperature: $A_{(g)} \rightleftharpoons B_{(g)} + C_{(g)}$. If $p$ is the total pressure,$K_p$ is the equilibrium constant,and $\alpha$ is the degree of dissociation,then which of the following is true at equilibrium?

MediumJEE MAIN 2025

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For a reaction $2 A \rightleftharpoons B + C$,$K_c$ is $2 \times 10^{-3}$. At a given time,the reaction mixture has $[A] = [B] = [C] = 3 \times 10^{-4} \ M$. Which of the following options is correct?

MediumTS EAMCET 2021

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$2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2_{(g)}}$. If $NOBr$ is $40\%$ dissociated at a certain temperature and a total pressure of $0.30 \text{ atm}$,the $K_p$ for the reaction $2NO_{(g)} + Br_{2_{(g)}} \rightleftharpoons 2NOBr_{(g)}$ is:

Medium

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The equilibrium constants $(K_C)$ of two reactions $H_2 + I_2 \rightleftharpoons 2 HI$ and $N_2 + 3 H_2 \rightleftharpoons 2 NH_3$ are $50$ and $1000$,respectively. The equilibrium constant of the reaction $N_2 + 6 HI \rightleftharpoons 2 NH_3 + 3 I_2$ is closest to

MediumKVPY 2014

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Consider a reversible reaction $2A + B \rightleftharpoons 2C$ having equilibrium constant $K_c = 25$. If a reaction vessel contains $2 \ mol$ of $A$,$0.25 \ mol$ of $B$,and $0.5 \ mol$ of $C$ in a $100 \ L$ vessel,what will be the direction of the reaction?

Similar Questions

For the reaction $SO_{2(g)} + NO_{2(g)} \rightleftharpoons SO_{3(g)} + NO_{(g)}$,the equilibrium constant $K_c$ is $16$. If $1 \ mol$ of each gas is taken in a $1 \ dm^3$ vessel,the equilibrium concentration of $NO$ will be ....

For a reaction $2 A \rightleftharpoons B + C$,$K_c$ is $2 \times 10^{-3}$. At a given time,the reaction mixture has $[A] = [B] = [C] = 3 \times 10^{-4} \ M$. Which of the following options is correct?

$2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2_{(g)}}$. If $NOBr$ is $40\%$ dissociated at a certain temperature and a total pressure of $0.30 \text{ atm}$,the $K_p$ for the reaction $2NO_{(g)} + Br_{2_{(g)}} \rightleftharpoons 2NOBr_{(g)}$ is:

The equilibrium constants $(K_C)$ of two reactions $H_2 + I_2 \rightleftharpoons 2 HI$ and $N_2 + 3 H_2 \rightleftharpoons 2 NH_3$ are $50$ and $1000$,respectively. The equilibrium constant of the reaction $N_2 + 6 HI \rightleftharpoons 2 NH_3 + 3 I_2$ is closest to

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