(D) The given reaction is $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$.The change in the number of moles of gaseous products and reactants is

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$1.44 \times 10^{-5} / (0.082 \times 773)^{-2}$

(D) The given reaction is $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$.The change in the number of moles of gaseous products and reactants is $\Delta n = 2 - (1 + 3) = -2$.The relationship between $K_p$ and $K_c$ is given by $K_p = K_c(RT)^{\Delta n}$.Substituting the values,$K_p = K_c(RT)^{-2}$.Therefore,$K_c = \frac{K_p}{(RT)^{-2}}$.Given $T = 500 \ ^oC = 500 + 273 = 773 \ K$ and $R = 0.082 \ \text{L atm K}^{-1} \text{mol}^{-1}$.Thus,$K_c = \frac{1.44 \times 10^{-5}}{(0.082 \times 773)^{-2}}$.

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Kp and Kc Relationship

Medium

For the reversible reaction,$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at $500 \ ^oC$,the value of $K_P$ is $1.44 \times 10^{-5}$ when partial pressure is measured in atmospheres. The corresponding value of $K_c$ with concentration in $\text{mol L}^{-1}$ is:

IIT 2000 All IIT

A
$1.44 \times 10^{-5} / (0.082 \times 500)^{-2}$
B
$1.44 \times 10^{-5} / (8.314 \times 773)^{-2}$
C
$1.44 \times 10^{-5} / (0.082 \times 773)^2$
D
$1.44 \times 10^{-5} / (0.082 \times 773)^{-2}$

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Kp and Kc Relationship

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For the reversible reaction,$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at $500 \ ^oC$,the value of $K_P$ is $1.44 \times 10^{-5}$ when partial pressure is measured in atmospheres. The corresponding value of $K_c$ with concentration in $\text{mol L}^{-1}$ is:

Similar Questions

Find the value of $\frac{P}{K_p}$ for the reaction at a certain temperature: $2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$,where $P$ is the total pressure of gases at equilibrium and $P_{Br_2} = \frac{P}{9}$.

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + \text{heat}$,which of the following relations is correct?

For the reaction $N_2O_{4_{(g)}} \rightleftharpoons 2NO_{2_{(g)}}$ at $298 \ K$,the equilibrium constant $K_p$ is $0.14 \ atm$. Calculate the value of $K_c$. $(R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1})$

At $444 \, ^\circ C$,the equilibrium constant for the reaction $HI \rightleftharpoons 1/2 H_2 + 1/2 I_2$ is $64$. What will be the equilibrium constant for the reaction $H_2 + I_2 \rightleftharpoons 2HI$?

For the reaction $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2}O_{2(g)}$,the equilibrium constant $K_C = 4.9 \times 10^{-2}$. Calculate the $K_C$ for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$.

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