(B) The relationship between the equilibrium constant in terms of concentration $(K_c)$ and partial pressure $(K_p)$ is given by the equation: $K_p =

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(B) The relationship between the equilibrium constant in terms of concentration $(K_c)$ and partial pressure $(K_p)$ is given by the equation: $K_p = K_c(RT)^{\Delta n}$ Here,$\Delta n$ is the change in the number of gaseous moles: $\Delta n = (2 + 1) - 2 = 1$ Given $K_c = 3.75 \times 10^{-6}$,$R = 0.082 \ L \ bar \ mol^{-1} \ K^{-1}$,and $T = 1069 \ K$: $K_p = 3.75 \times 10^{-6} \times (0.082 \times 1069)^{1}$ $K_p = 3.75 \times 10^{-6} \times 87.658$ $K_p \approx 3.287 \times 10^{-4}$ Rounding to two significant figures,we get $K_p \approx 3.3 \times 10^{-4}$.

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

Medium

For a reaction $2A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$,$K_c = 3.75 \times 10^{-6}$ at $1069 \ K$. The approximate value of $K_p$ for this reaction at the same temperature is $(R = 0.082 \ L \ bar \ mol^{-1} \ K^{-1})$.

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A
$2.4 \times 10^{-4}$
B
$3.3 \times 10^{-4}$
C
$33 \times 10^2$
D
$7.2 \times 10^{34}$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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The value of $K_{p}$ for the reaction,$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$ is $3.0$ at $1000 \ K$. If initially $P_{CO_{2}} = 0.48 \ bar$ and $P_{CO} = 0 \ bar$ and pure graphite is present,calculate the equilibrium partial pressures of $CO$ and $CO_{2}$.

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MediumJEE MAIN 2023

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For the reaction: $HI_{(g)} \rightleftharpoons \frac{1}{2}H_{2(g)} + \frac{1}{2}I_{2(g)}$,the equilibrium constant is $8$. What is the equilibrium constant for the reaction: $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$?

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For a reaction $2A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$,$K_c = 3.75 \times 10^{-6}$ at $1069 \ K$. The approximate value of $K_p$ for this reaction at the same temperature is $(R = 0.082 \ L \ bar \ mol^{-1} \ K^{-1})$.

Similar Questions

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,$1 mol$ of $PCl_5$ is taken at $5 atm$ pressure. If $50\%$ of $PCl_5$ dissociates at equilibrium,calculate $K_p$.

The value of $K_{p}$ for the reaction,$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$ is $3.0$ at $1000 \ K$. If initially $P_{CO_{2}} = 0.48 \ bar$ and $P_{CO} = 0 \ bar$ and pure graphite is present,calculate the equilibrium partial pressures of $CO$ and $CO_{2}$.

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 .......

Water decomposes at $2300 \ K$. $H_2O_{(g)} \rightleftharpoons H_{2(g)} + \frac{1}{2} O_{2(g)}$. The percent of water decomposing at $2300 \ K$ and $1 \ bar$ is $...........$ (Nearest integer). Equilibrium constant for the reaction is $2 \times 10^{-3}$ at $2300 \ K$.

For the reaction: $HI_{(g)} \rightleftharpoons \frac{1}{2}H_{2(g)} + \frac{1}{2}I_{2(g)}$,the equilibrium constant is $8$. What is the equilibrium constant for the reaction: $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$?

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