(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 $(R = 0.082 \ L \ bar \ mol^{-1} \ K^{-1})$.

TS EAMCET 2018 All TS EAMCET

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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At $1000 \ K$,if the equilibrium constant $K_p$ for the reaction $2 \ NOCl_{(g)} \rightleftharpoons 2 \ NO_{(g)} + Cl_{2(g)}$ is $4.157 \times 10^{-4} \ bar$,the $K_c$ (in $mol \ L^{-1}$) is $(R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1})$

MediumAP EAMCET 2018

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$2 \ mol$ of $PCl_5$ is heated in a closed vessel of $2 \ L$ capacity. When equilibrium is attained,$PCl_5$ is $40\%$ dissociated. The equilibrium constant $K_c$ for the reaction will be ........... $mol/L$.

Difficult

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The values of $K_p/K_c$ for the following reactions at $300 \ K$ are respectively (At $300 \ K, RT = 24.62 \ dm^3 \ atm \ mol^{-1}$):
$(i) \ N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$
$(ii) \ N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$
$(iii) \ N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

DifficultJEE MAIN 2019

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For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the value of $K_p = 41$ at $400 \ K$. Find out the value of $K_p$ for the following reaction at the same temperature: $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$

Medium

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In which of the following plots,an endothermic reaction is correctly represented?

DifficultTS EAMCET 2019

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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

At $1000 \ K$,if the equilibrium constant $K_p$ for the reaction $2 \ NOCl_{(g)} \rightleftharpoons 2 \ NO_{(g)} + Cl_{2(g)}$ is $4.157 \times 10^{-4} \ bar$,the $K_c$ (in $mol \ L^{-1}$) is $(R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1})$

$2 \ mol$ of $PCl_5$ is heated in a closed vessel of $2 \ L$ capacity. When equilibrium is attained,$PCl_5$ is $40\%$ dissociated. The equilibrium constant $K_c$ for the reaction will be ........... $mol/L$.

The values of $K_p/K_c$ for the following reactions at $300 \ K$ are respectively (At $300 \ K, RT = 24.62 \ dm^3 \ atm \ mol^{-1}$):$(i) \ N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$$(ii) \ N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$$(iii) \ N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the value of $K_p = 41$ at $400 \ K$. Find out the value of $K_p$ for the following reaction at the same temperature: $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$

In which of the following plots,an endothermic reaction is correctly represented?

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