(C) Initial moles: $n(PCl_{5}) = 5$,$n(N_{2}) = 2$. Total moles at equilibrium: $n_{total} = (5-x) + x + x + 2 = 7+x$.Using ideal gas law $PV = nRT$ a

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(C) Initial moles: $n(PCl_{5}) = 5$,$n(N_{2}) = 2$. Total moles at equilibrium: $n_{total} = (5-x) + x + x + 2 = 7+x$.Using ideal gas law $PV = nRT$ at equilibrium:$2.46 \times 200 = (7+x) \times 0.082 \times 600$$492 = (7+x) \times 49.2$$7+x = 10 \implies x = 3$.At equilibrium: $n(PCl_{5}) = 2$,$n(PCl_{3}) = 3$,$n(Cl_{2}) = 3$,$n(N_{2}) = 2$. Total moles $= 10$.Partial pressures: $P(PCl_{5}) = (2/10) \times 2.46 = 0.492 \, atm$,$P(PCl_{3}) = (3/10) \times 2.46 = 0.738 \, atm$,$P(Cl_{2}) = (3/10) \times 2.46 = 0.738 \, atm$.$K_{p} = \frac{P(PCl_{3}) \times P(Cl_{2})}{P(PCl_{5})} = \frac{0.738 \times 0.738}{0.492} = 1.107$.$K_{p} = 1107 \times 10^{-3}$.

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

Medium

$PCl_{5}$ dissociates as $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$. $5 \, \text{moles}$ of $PCl_{5}$ are placed in a $200 \, L$ vessel which contains $2 \, \text{moles}$ of $N_{2}$ and is maintained at $600 \, K$. The equilibrium pressure is $2.46 \, atm$. The equilibrium constant $K_{p}$ for the dissociation of $PCl_{5}$ is $...... \times 10^{-3}$. (nearest integer) (Given: $R = 0.082 \, L \, atm \, K^{-1} \, mol^{-1}$: Assume ideal gas behaviour)

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$2312$
B
$954$
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$1107$
D
$1451$

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

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The equilibrium composition for the reaction $PCl_3 + Cl_2 \rightleftharpoons PCl_5$ at $298 \, K$ is given below.
$[PCl_3]_{eq} = 0.2 \, mol \, L^{-1}$
$[Cl_2]_{eq} = 0.1 \, mol \, L^{-1}$
$[PCl_5]_{eq} = 0.40 \, mol \, L^{-1}$
If $0.2 \, mol$ of $Cl_2$ is added at the same temperature,the equilibrium concentration of $PCl_5$ is $.... \times 10^{-2} \, mol \, L^{-1}$. Given: $K_c$ for the reaction at $298 \, K$ is $20$.

MediumJEE MAIN 2023

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$10 \%$ of $PCl_5$ decomposes at a definite temperature and $4 \ atm$ pressure. At the same temperature,if $20 \%$ of $PCl_5$ decomposes,find the pressure. (Temperature remains constant.) (in $atm$)

Difficult

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For the reaction $Br_2 \rightleftharpoons 2Br$,the equilibrium constants at $327\,^oC$ and $527\,^oC$ are $6.1 \times 10^{-12}$ and $1.0 \times 10^{-7}$ respectively. The reaction is ...........

Easy

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The reaction $2 NO_{2(g)} \rightleftharpoons N_2O_{4(g)}$ is at equilibrium in a closed $15 \ L$ vessel at $300 \ K$. The total weight of the mixture of $NO_2$ and $N_2O_4$ in the vessel is $64.4 \ g$. The equilibrium constant for the reaction is $K_p = 6.67$. Assuming ideal gas behavior,the total pressure in the vessel (in $atm$) is: [Given: Gas constant $R = 0.082 \ atm \ L \ K^{-1} \ mol^{-1}$]

MediumKVPY 2021

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The equilibrium constant at $298 \ K$ for a reaction $A + B \rightleftharpoons C + D$ is $100$. If the initial concentration of all the four species were $1 \ M$ each,then the equilibrium concentration of $D$ (in $mol \ L^{-1}$) will be:

DifficultJEE MAIN 2016

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$10 \%$ of $PCl_5$ decomposes at a definite temperature and $4 \ atm$ pressure. At the same temperature,if $20 \%$ of $PCl_5$ decomposes,find the pressure. (Temperature remains constant.) (in $atm$)

For the reaction $Br_2 \rightleftharpoons 2Br$,the equilibrium constants at $327\,^oC$ and $527\,^oC$ are $6.1 \times 10^{-12}$ and $1.0 \times 10^{-7}$ respectively. The reaction is ...........

The equilibrium constant at $298 \ K$ for a reaction $A + B \rightleftharpoons C + D$ is $100$. If the initial concentration of all the four species were $1 \ M$ each,then the equilibrium concentration of $D$ (in $mol \ L^{-1}$) will be:

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