(A) For the given reaction,$\Delta n = 2 - 3 = -1$.Given: $T = 450 \, K$,$R = 0.0831 \, L \, bar \, K^{-1} \, mol^{-1}$,$K_{p} = 2.0 \times 10^{10} \,

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$7.48 \times 10^{11} \, M^{-1}$

(A) For the given reaction,$\Delta n = 2 - 3 = -1$.Given: $T = 450 \, K$,$R = 0.0831 \, L \, bar \, K^{-1} \, mol^{-1}$,$K_{p} = 2.0 \times 10^{10} \, bar^{-1}$.The relationship between $K_{p}$ and $K_{c}$ is $K_{p} = K_{c}(RT)^{\Delta n}$.Substituting the values: $2.0 \times 10^{10} = K_{c} (0.0831 \times 450)^{-1}$.$K_{c} = 2.0 \times 10^{10} \times (0.0831 \times 450) = 2.0 \times 10^{10} \times 37.395$.$K_{c} = 74.79 \times 10^{10} = 7.48 \times 10^{11} \, M^{-1}$.

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

Medium

At $450 \, K$,$K_{p} = 2.0 \times 10^{10} \, bar^{-1}$ for the given reaction at equilibrium.
$2 \, SO_{2(g)} + O_{2(g)} \longleftrightarrow 2 \, SO_{3(g)}$
What is $K_{c}$ at this temperature?

A
$7.48 \times 10^{11} \, M^{-1}$
B
$2.0 \times 10^{10} \, M^{-1}$
C
$5.35 \times 10^{8} \, M^{-1}$
D
$7.48 \times 10^{10} \, M^{-1}$

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Kp and Kc Relationship

One mole of $SO_3$ was placed in a $1 \ L$ reaction vessel at a certain temperature. The following equilibrium was established: $2SO_3 \rightleftharpoons 2SO_2 + O_2$. At equilibrium,$0.6 \ moles$ of $SO_2$ were formed. The equilibrium constant $(K_c)$ of the reaction will be:

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For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$,the equilibrium constant is $K$. What will be the equilibrium constant for the reaction $NH_3 \rightleftharpoons \frac{1}{2}N_2 + \frac{3}{2}H_2$?

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For the reactions $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ and $\frac{1}{2}N_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons NO_{(g)}$,if the equilibrium constants are $K_1$ and $K_2$ respectively,then their relationship is:

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At $450 \, K$,$K_{p} = 2.0 \times 10^{10} \, bar^{-1}$ for the given reaction at equilibrium.$2 \, SO_{2(g)} + O_{2(g)} \longleftrightarrow 2 \, SO_{3(g)}$What is $K_{c}$ at this temperature?

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One mole of $SO_3$ was placed in a $1 \ L$ reaction vessel at a certain temperature. The following equilibrium was established: $2SO_3 \rightleftharpoons 2SO_2 + O_2$. At equilibrium,$0.6 \ moles$ of $SO_2$ were formed. The equilibrium constant $(K_c)$ of the reaction will be:

One mole of $PCl_5$ is heated in a closed vessel of $1 \ L$ capacity. At equilibrium,$20\%$ of $PCl_5$ remains undissociated. Find the value of $K_c$.

If the degree of dissociation is $\sqrt{0.5}$,what will be the value of $K_p$ for the reaction $N_2O_3 \rightleftharpoons NO + NO_2$ in terms of the total pressure $P$?

For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$,the equilibrium constant is $K$. What will be the equilibrium constant for the reaction $NH_3 \rightleftharpoons \frac{1}{2}N_2 + \frac{3}{2}H_2$?

For the reactions $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ and $\frac{1}{2}N_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons NO_{(g)}$,if the equilibrium constants are $K_1$ and $K_2$ respectively,then their relationship is:

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At $450 \, K$,$K_{p} = 2.0 \times 10^{10} \, bar^{-1}$ for the given reaction at equilibrium.
$2 \, SO_{2(g)} + O_{2(g)} \longleftrightarrow 2 \, SO_{3(g)}$
What is $K_{c}$ at this temperature?