(C) The equilibrium constant expression for the reaction $PCl_5 \rightleftharpoons PCl_3 + Cl_2$ is $K_p = \frac{p_{PCl_3} \times p_{Cl_2}}{p_{PCl_5}}

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(C) The equilibrium constant expression for the reaction $PCl_5 \rightleftharpoons PCl_3 + Cl_2$ is $K_p = \frac{p_{PCl_3} \times p_{Cl_2}}{p_{PCl_5}}$.Initially,$K_p = \frac{0.3 \times 0.2}{0.6} = \frac{0.06}{0.6} = 0.1$.When the partial pressures of $PCl_3$ and $Cl_2$ are doubled,the new partial pressures are $p'_{PCl_3} = 2 \times 0.3 = 0.6 \ atm$ and $p'_{Cl_2} = 2 \times 0.2 = 0.4 \ atm$.Let the new partial pressure of $PCl_5$ be $x$.Since $K_p$ remains constant at $0.1$,we have $0.1 = \frac{0.6 \times 0.4}{x}$.Solving for $x$: $x = \frac{0.24}{0.1} = 2.4 \ atm$.

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

Medium

In the reaction $PCl_5 \rightleftharpoons PCl_3 + Cl_2$,the partial pressures of $PCl_3$,$Cl_2$,and $PCl_5$ are $0.3 \ atm$,$0.2 \ atm$,and $0.6 \ atm$ respectively. If the partial pressures of $PCl_3$ and $Cl_2$ are doubled,what will be the partial pressure of $PCl_5$ in $atm$?

A
$0.3$
B
$1.2$
C
$2.4$
D
$0.15$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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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If $0.5 \ mol$ of $H_2$ and $0.5 \ mol$ of $I_2$ are reacted in a $10 \ L$ vessel at $444 \ ^\circ C$,and the equilibrium constant $K_c$ at the same temperature is $49$,then the ratio of $[HI]$ to $[I_2]$ is .......

Medium

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One mole $H_2O_{(g)}$ and one mole $CO_{(g)}$ are taken in a $1 \ L$ flask and heated to $725 \ K$. At equilibrium,$40 \%$ (by mass) of water reacted with $CO_{(g)}$ as follows: $H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2_{(g)}} + CO_{2_{(g)}}$. The value of $K_p$ is:

MediumAP EAMCET 2023

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For the reaction ${N_{2(g)}} + {O_{2(g)}} \rightleftharpoons 2NO_{(g)}$,the value of $K_c$ at $400 \ K$ is $4.0 \times 10^{-6}$. The value of $K_p$ for this reaction is .....

Medium

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For the reaction $3A_{(g)} + B_{(g)} \rightleftharpoons 2C_{(g)}$ at a given temperature,$K_c$ is $9.0$. What must be the volume of the flask if a mixture of $2.0 \ mol$ each of $A, B$ and $C$ is obtained at equilibrium? .....$L$

Medium

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In the reaction $PCl_5 \rightleftharpoons PCl_3 + Cl_2$,the partial pressures of $PCl_3$,$Cl_2$,and $PCl_5$ are $0.3 \ atm$,$0.2 \ atm$,and $0.6 \ atm$ respectively. If the partial pressures of $PCl_3$ and $Cl_2$ are doubled,what will be the partial pressure of $PCl_5$ in $atm$?

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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?

If $0.5 \ mol$ of $H_2$ and $0.5 \ mol$ of $I_2$ are reacted in a $10 \ L$ vessel at $444 \ ^\circ C$,and the equilibrium constant $K_c$ at the same temperature is $49$,then the ratio of $[HI]$ to $[I_2]$ is .......

One mole $H_2O_{(g)}$ and one mole $CO_{(g)}$ are taken in a $1 \ L$ flask and heated to $725 \ K$. At equilibrium,$40 \%$ (by mass) of water reacted with $CO_{(g)}$ as follows: $H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2_{(g)}} + CO_{2_{(g)}}$. The value of $K_p$ is:

For the reaction ${N_{2(g)}} + {O_{2(g)}} \rightleftharpoons 2NO_{(g)}$,the value of $K_c$ at $400 \ K$ is $4.0 \times 10^{-6}$. The value of $K_p$ for this reaction is .....

For the reaction $3A_{(g)} + B_{(g)} \rightleftharpoons 2C_{(g)}$ at a given temperature,$K_c$ is $9.0$. What must be the volume of the flask if a mixture of $2.0 \ mol$ each of $A, B$ and $C$ is obtained at equilibrium? .....$L$

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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?