For which one of the following reactions is K | vedclass

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(B) The relationship between $K_p$ and $K_c$ is given by the equation $K_p = K_c(RT)^{\Delta n_g}$,where $\Delta n_g$ is the change in the number of m

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$N_2(g) + O_2(g) \rightleftharpoons 2NO(g)$

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(B) The relationship between $K_p$ and $K_c$ is given by the equation $K_p = K_c(RT)^{\Delta n_g}$,where $\Delta n_g$ is the change in the number of moles of gaseous products and reactants.For $K_p = K_c$,the exponent $\Delta n_g$ must be equal to $0$.Calculating $\Delta n_g$ for each reaction:$A$: $\Delta n_g = 2 - (1 + 3) = -2$$B$: $\Delta n_g = 2 - (1 + 1) = 0$$C$: $\Delta n_g = (1 + 1) - 1 = 1$$D$: $\Delta n_g = (2 + 1) - 2 = 1$Since $\Delta n_g = 0$ for reaction $B$,$K_p = K_c$ for this reaction.

For which one of the following reactions is $K_p = K_c$?

Similar Questions

At $413 \ K$ temperature and $100 \ atm$ pressure,$1 \ mol$ $N_2$ and $3 \ mol$ $H_2$ are heated in a closed vessel. At equilibrium,$0.50 \ mol$ $NH_3$ is present. Find $K_p$.

For the reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$ at $25^o C$,the value of $K_c$ is $6.10 \times 10^{-3}$. What is the value of $K_c$ for the equilibrium reaction $NO_{2(g)} \rightleftharpoons 1/2 N_2O_{4(g)}$?

Given the equilibria:
$I: A + 2B \rightleftharpoons C ; K_{eq} = K_1$
$II: C + D \rightleftharpoons 3A ; K_{eq} = K_2$
$III: 6B + D \rightleftharpoons 2C ; K_{eq} = K_3$
Which of the following relations is correct?

For the reaction ${N_2}_{(g)} + {O_2}_{(g)} \rightleftharpoons 2NO_{(g)}$,the equilibrium constant ${K_C}$ is $4 \times 10^{-4}$ at temperature $T$. Calculate ${K_P}$.

Calculate $K_{C}$ for the reversible process given below if $K_{P}=167$ and $T=800^{\circ}C$.
$CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$

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