(C) For the reaction: $A_2B_{6(g)} \rightleftharpoons A_2B_{4(g)} + B_{2(g)}$Initial pressure: $P_{A_2B_6} = 4 \text{ atm}$At equilibrium: $P_{A_2B_6}

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(C) For the reaction: $A_2B_{6(g)} \rightleftharpoons A_2B_{4(g)} + B_{2(g)}$Initial pressure: $P_{A_2B_6} = 4 \text{ atm}$At equilibrium: $P_{A_2B_6} = 4 - x$,$P_{A_2B_4} = x$,$P_{B_2} = x$$K_p = \frac{P_{A_2B_4} \cdot P_{B_2}}{P_{A_2B_6}} = \frac{x^2}{4-x} = 0.04$$x^2 = 0.16 - 0.04x$$x^2 + 0.04x - 0.16 = 0$Solving the quadratic equation: $x = \frac{-0.04 + \sqrt{(0.04)^2 - 4(1)(-0.16)}}{2} \approx 0.38 \text{ atm}$Equilibrium pressure of $A_2B_6 = 4 - x = 4 - 0.38 = 3.62 \text{ atm}$.

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

Medium

At $T(K)$,the $K_p$ for the reaction $A_2B_{6(g)} \rightleftharpoons A_2B_{4(g)} + B_{2(g)}$ is $0.04 \text{ atm}$. The equilibrium pressure (in $\text{atm}$) of $A_2B_{6(g)}$ when it is placed in a flask at $4 \text{ atm}$ pressure and allowed to come to equilibrium is:

AP EAMCET 2023 All AP EAMCET

A
$0.362$
B
$0.380$
C
$3.62$
D
$2.62$

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6-1.Equilibrium (Chemical Equilibrium)

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

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At $T \ K$,$K_{c}$ for the reaction $SO_{2(g)} + NO_{2(g)} \rightleftharpoons SO_{3(g)} + NO_{(g)}$ is $16$. If initially one mole each of all the four gases are taken in a $1 \ L$ vessel,the equilibrium concentrations of $SO_{3(g)}$ and $SO_{2(g)}$ in $mol \ L^{-1}$ respectively are:

MediumAP EAMCET 2017

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For the reaction,$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,if dinitrogen tetroxide is $50\%$ dissociated at $60^\circ C$,the standard free energy change at this temperature and $1 \ atm$ pressure is:

MediumAP EAMCET 2020

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Which of the following is correct for the equilibrium shown below?
$2CH_3COOH \rightleftharpoons (CH_3COOH)_2$
(Equilibrium constants for the reaction in water and benzene are $K_{Water}$ and $K_{Benzene}$ respectively.)

Difficult

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The following reaction is performed at $298 \, K$.
$2 NO_{(g)} + O_{2(g)} \rightleftharpoons 2 NO_{2(g)}$
The standard free energy of formation of $NO_{(g)}$ is $86.6 \, kJ/mol$ at $298 \, K$. What is the standard free energy of formation of $NO_{2(g)}$ at $298 \, K$? $(K_p = 1.6 \times 10^{12})$

JEE MAIN 2015

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For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,the value of $K_c$ is $0.04$ at $250 \ ^oC$ in a $3 \ L$ vessel. If the concentration of $Cl_2$ at equilibrium is $0.15 \ M$,then the initial moles of $PCl_5$ will be ...........

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At $T(K)$,the $K_p$ for the reaction $A_2B_{6(g)} \rightleftharpoons A_2B_{4(g)} + B_{2(g)}$ is $0.04 \text{ atm}$. The equilibrium pressure (in $\text{atm}$) of $A_2B_{6(g)}$ when it is placed in a flask at $4 \text{ atm}$ pressure and allowed to come to equilibrium is:

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At $T \ K$,$K_{c}$ for the reaction $SO_{2(g)} + NO_{2(g)} \rightleftharpoons SO_{3(g)} + NO_{(g)}$ is $16$. If initially one mole each of all the four gases are taken in a $1 \ L$ vessel,the equilibrium concentrations of $SO_{3(g)}$ and $SO_{2(g)}$ in $mol \ L^{-1}$ respectively are:

For the reaction,$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,if dinitrogen tetroxide is $50\%$ dissociated at $60^\circ C$,the standard free energy change at this temperature and $1 \ atm$ pressure is:

Which of the following is correct for the equilibrium shown below?$2CH_3COOH \rightleftharpoons (CH_3COOH)_2$(Equilibrium constants for the reaction in water and benzene are $K_{Water}$ and $K_{Benzene}$ respectively.)

The following reaction is performed at $298 \, K$.$2 NO_{(g)} + O_{2(g)} \rightleftharpoons 2 NO_{2(g)}$The standard free energy of formation of $NO_{(g)}$ is $86.6 \, kJ/mol$ at $298 \, K$. What is the standard free energy of formation of $NO_{2(g)}$ at $298 \, K$? $(K_p = 1.6 \times 10^{12})$

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,the value of $K_c$ is $0.04$ at $250 \ ^oC$ in a $3 \ L$ vessel. If the concentration of $Cl_2$ at equilibrium is $0.15 \ M$,then the initial moles of $PCl_5$ will be ...........

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Which of the following is correct for the equilibrium shown below?
$2CH_3COOH \rightleftharpoons (CH_3COOH)_2$
(Equilibrium constants for the reaction in water and benzene are $K_{Water}$ and $K_{Benzene}$ respectively.)

The following reaction is performed at $298 \, K$.
$2 NO_{(g)} + O_{2(g)} \rightleftharpoons 2 NO_{2(g)}$
The standard free energy of formation of $NO_{(g)}$ is $86.6 \, kJ/mol$ at $298 \, K$. What is the standard free energy of formation of $NO_{2(g)}$ at $298 \, K$? $(K_p = 1.6 \times 10^{12})$