(B) The relationship between standard Gibbs free energy change and the equilibrium constant is given by the equation: $\Delta_r G^{\ominus} = -RT \ln

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(B) The relationship between standard Gibbs free energy change and the equilibrium constant is given by the equation: $\Delta_r G^{\ominus} = -RT \ln K_{eq}$.Given: $\Delta_r G^{\ominus} = 165.469 \ kJ \ mol^{-1} = 165469 \ J \ mol^{-1}$,$T = 298 \ K$,and $R = 8.3 \ J \ mol^{-1} \ K^{-1}$.Substituting the values: $165469 = -(8.3) \times (298) \times \ln K_{eq}$.$\ln K_{eq} = -\frac{165469}{8.3 \times 298} = -\frac{165469}{2473.4} \approx -66.9$.$K_{eq} = e^{-66.9} \approx 10^{-29}$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Standard free energy

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At $298 \ K$,$\Delta_r G^{\ominus}$ for the following reaction is $165.469 \ kJ \ mol^{-1}$. What is the equilibrium constant for this reaction? $(R = 8.3 \ J \ mol^{-1} \ K^{-1})$
$\frac{3}{2} O_{2(g)} \longrightarrow O_{3(g)}$

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A
$10^{29}$
B
$10^{-29}$
C
$5 \times 10^{-27}$
D
$5 \times 10^{+27}$

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6-1.Equilibrium (Chemical Equilibrium)

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Standard free energy

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At $298 \ K$,$\Delta_r G^{\ominus}$ for the following reaction is $165.469 \ kJ \ mol^{-1}$. What is the equilibrium constant for this reaction? $(R = 8.3 \ J \ mol^{-1} \ K^{-1})$$\frac{3}{2} O_{2(g)} \longrightarrow O_{3(g)}$

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Given $\Delta G^o (HI, g) \cong + 1.7 \ kJ \ mol^{-1}$. What is the equilibrium constant at $25 ^oC$ for the reaction $2HI_{(g)} \rightleftharpoons H_{2_{(g)}} + I_{2_{(g)}}$?

Find the value of the equilibrium constant $(K)$ of a reaction at $300 \ K$,when standard Gibbs free energy change is $-25 \ kJ \ mol^{-1}$? (Consider $R = 8.33 \ J \ mol^{-1} \ K^{-1}$)

The equilibrium concentrations of the species in the reaction $A + B \rightleftharpoons C + D$ are $3, 5, 10$ and $15 \ mol \ L^{-1}$ respectively at $300 \ K$. The $\Delta G$ for the reaction is (in $cal$)

Hydrolysis of sucrose gives,$Sucrose + H_{2}O \rightleftharpoons Glucose + Fructose$Equilibrium constant $K_{c}$ for the reaction is $2 \times 10^{13}$ at $300 \ K$. Calculate $\Delta G^{\ominus}$ at $300 \ K$.

For the reaction taking place at a certain temperature $NH_2COONH_{4(s)} \rightleftharpoons 2NH_{3(g)} + CO_{2(g)}$,if the equilibrium pressure is $X \ bar$,then $\Delta_r G^o$ would be :-

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At $298 \ K$,$\Delta_r G^{\ominus}$ for the following reaction is $165.469 \ kJ \ mol^{-1}$. What is the equilibrium constant for this reaction? $(R = 8.3 \ J \ mol^{-1} \ K^{-1})$
$\frac{3}{2} O_{2(g)} \longrightarrow O_{3(g)}$

Hydrolysis of sucrose gives,
$Sucrose + H_{2}O \rightleftharpoons Glucose + Fructose$
Equilibrium constant $K_{c}$ for the reaction is $2 \times 10^{13}$ at $300 \ K$. Calculate $\Delta G^{\ominus}$ at $300 \ K$.