(C) The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n_g}$.For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3

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(C) The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n_g}$.For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the change in the number of moles of gas is $\Delta n_g = 2 - (1 + 3) = -2$.Given $T = 300 + 273 = 573 \, K$,$K_c = 0.65$,and $R = 0.082 \, L \cdot atm \cdot K^{-1} \cdot mol^{-1}$.Substituting these values: $K_p = 0.65 \times (0.082 \times 573)^{-2}$.$K_p = 0.65 \times (46.986)^{-2} = 0.65 \times (1 / 2207.68) \approx 2.94 \times 10^{-4}$.

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

Medium

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at $300 \, ^\circ C$,the value of $K_c$ is $0.65$. If $R = 0.082 \, L \cdot atm \cdot K^{-1} \cdot mol^{-1}$,then the value of $K_p$ will be:

A
$0.29 \times 10^{-4}$
B
$29 \times 10^{-4}$
C
$2.9 \times 10^{-4}$
D
$0.029 \times 10^{-4}$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

At $500 \ K$,for the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the $K_p$ is $0.036 \ atm^{-2}$. What is its $K_C$ in $L^2 \ mol^{-2}$? $(R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1})$.

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For which of the following reactions is the relation $\frac{K_p}{K_c} + \log(RT) = 0$ correct?

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For the reactions $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ and $NO_{(g)} \rightleftharpoons 1/2N_{2(g)} + 1/2O_{2(g)}$,the equilibrium constants are $K_1$ and $K_2$ respectively. What is the relationship between $K_1$ and $K_2$?

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The half-life of forward and reverse reactions are $400 \, sec$ and $100 \, sec$ respectively. If these half-lives are independent of the concentration of the reactant,find the equilibrium constant of the reaction.

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For the reaction $P + Q \rightleftharpoons R + C$,the equilibrium constant $K_c$ is $10^{-2}$ and the forward rate constant $K_f$ is $10^{-1}$. The rate constant for the backward reaction $(K_b)$ will be:

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For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at $300 \, ^\circ C$,the value of $K_c$ is $0.65$. If $R = 0.082 \, L \cdot atm \cdot K^{-1} \cdot mol^{-1}$,then the value of $K_p$ will be:

Similar Questions

At $500 \ K$,for the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the $K_p$ is $0.036 \ atm^{-2}$. What is its $K_C$ in $L^2 \ mol^{-2}$? $(R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1})$.

For which of the following reactions is the relation $\frac{K_p}{K_c} + \log(RT) = 0$ correct?

For the reactions $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ and $NO_{(g)} \rightleftharpoons 1/2N_{2(g)} + 1/2O_{2(g)}$,the equilibrium constants are $K_1$ and $K_2$ respectively. What is the relationship between $K_1$ and $K_2$?

The half-life of forward and reverse reactions are $400 \, sec$ and $100 \, sec$ respectively. If these half-lives are independent of the concentration of the reactant,find the equilibrium constant of the reaction.

For the reaction $P + Q \rightleftharpoons R + C$,the equilibrium constant $K_c$ is $10^{-2}$ and the forward rate constant $K_f$ is $10^{-1}$. The rate constant for the backward reaction $(K_b)$ will be:

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