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11th
Chemistry
Equilibrium
$Relationship between Equilibrium Constant, Reaction Quotient and Gibbs Energy$

Relationship between Equilibrium Constant, Reaction Quotient and Gibbs Energy

Equilibrium

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Relation Between Gibbs Free Energy and Equillibrium Constant

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Law of Chemical Equilibrium, Equilibrium Constant - Examples Nernst equation: Concepts, Derivation, Conditions, Example and Videos Spontaneity: Definition, Prediction, Gibbs Energy, Videos, Solved Example

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Relation Between Gibbs Free Energy and Equillibrium Constant

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Relating Equilibrium Constant, Reaction Quotient and Gibbs Free Energy

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A vessel contains three gases A, B and C in the equilibrium:

$A ⇌ 2 B + C$

At equilibrium, the concentration of A was $3$ M and that of B was $4$ M. On doubling the volume of the vessel, the new equilibrium concentration of B was $3$ M. Calculate $K_{c}$ and the initial equilibrium concentration of C.

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A reaction mixture containing $H_{2}, N_{2}$ and $N H_{3}$ has partial pressure 2 atm, 1atm and 3 atm respectively at 725 K. If the value of K for the reaction. $N_{2} + 3 H_{2} ⇌ 2 N H_{3}$ is $4.28 \times 1 0^{- 5}$
atm $^{- 2}$ at 725 K, in which direction the net reaction will go:

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$△ G^{\circ}$ for $\frac{1}{2} N_{2} + \frac{3}{2} H_{2} ⇌ N H_{3}$ is $- 16.5 k J m o l^{- 1}$ at $2 5^{\circ} C$ . Find out $K_{p}$ for the reaction. Also report $K_{p}$ and $△ G^{\circ}$ for:

$N_{2} + 3 H_{2} \to 2 N H_{3}$ at $2 5^{\circ} C$ .

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The equilibrium constant of a reaction doubles on increasing the temperature of the reaction from $2 5^{o} C$ to $3 5^{o} C$ . Calculate enthalpy change of the reaction, assuming it to be constant in this temperature range.

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Density of equilibrium mixture of $N_{2} O$ and $N O_{2}$ at 1 atm and 384 K is $1.84 g / d m^{3}$ . Equilibrium constant of the following reaction is:
$N_{2} O_{4} ⇌ 2 N O_{2}$

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1 mole of $P C l_{3}$ and 1 mole of $P C l_{5}$ is taken in a vessel of 10 L capacity maintained at 400 K.At equilibrium, the moles of $C l_{2}$ is found to be $4 \times 1 0^{- 3}$

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Steam undergoes decomposition at high temperature as per the reaction
$H_{2} O (g) ⇌ H_{2} (g) + \frac{1}{2} O_{2} (g), Δ H^{\circ} = 200 k J m o l^{- 1} Δ S^{\circ} = 40 J m o l^{- 1}$
The temperature at which equilibrium constant is unit is :

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Calculate value of $^{'} l n (K_{e q})$ ' for the reaction at 250 K.
$N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)$
Given: $H_{f}^{0} ((N O_{2}) g) = + 40.407 k J / m o l$
$H_{f}^{0} ((N_{2} O_{4}) g) = + 70 k J / m o l$
$S_{r}^{0} = 10 J K^{- 1}$

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At 473 K, $K_{c}$ for the reaction:
$P C l_{5 (g)} ⇌ P C l_{3 (g)} + C l_{2 (g)}$ is $8.3 \times 1 0^{- 3}$ .

What will be the value of $K_{c}$ , for the formation of $P C l_{5 (g)}$ at the same temperature?

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$1$ mole of $N O$ and $1$ mole of $O_{3}$ are taken in a $10 L$ vessel and heated. At equilibrium, $50 %$ of $N O$ (by mass) reacts with $O_{3}$ according to the equation:

$N O_{(g)} + O_{3 (g)} ⇌ N O_{2 (g)} + O_{2 (g)}$

What will be the equilibrium constant for this reaction?

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Relationship between Equilibrium Constant, Reaction Quotient and Gibbs Energy

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Relation Between Gibbs Free Energy and Equillibrium Constant

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Relating Equilibrium Constant, Reaction Quotient and Gibbs Free Energy

Related questions

A reaction mixture containing $H_{2}, N_{2}$ and $N H_{3}$ has partial pressure 2 atm, 1atm and 3 atm respectively at 725 K. If the value of K for the reaction. $N_{2} + 3 H_{2} ⇌ 2 N H_{3}$ is $4.28 \times 1 0^{- 5}$
atm $^{- 2}$ at 725 K, in which direction the net reaction will go:

$△ G^{\circ}$ for $\frac{1}{2} N_{2} + \frac{3}{2} H_{2} ⇌ N H_{3}$ is $- 16.5 k J m o l^{- 1}$ at $2 5^{\circ} C$ . Find out $K_{p}$ for the reaction. Also report $K_{p}$ and $△ G^{\circ}$ for:

$N_{2} + 3 H_{2} \to 2 N H_{3}$ at $2 5^{\circ} C$ .

The equilibrium constant of a reaction doubles on increasing the temperature of the reaction from $2 5^{o} C$ to $3 5^{o} C$ . Calculate enthalpy change of the reaction, assuming it to be constant in this temperature range.

Density of equilibrium mixture of $N_{2} O$ and $N O_{2}$ at 1 atm and 384 K is $1.84 g / d m^{3}$ . Equilibrium constant of the following reaction is:
$N_{2} O_{4} ⇌ 2 N O_{2}$

1 mole of $P C l_{3}$ and 1 mole of $P C l_{5}$ is taken in a vessel of 10 L capacity maintained at 400 K.At equilibrium, the moles of $C l_{2}$ is found to be $4 \times 1 0^{- 3}$

Steam undergoes decomposition at high temperature as per the reaction
$H_{2} O (g) ⇌ H_{2} (g) + \frac{1}{2} O_{2} (g), Δ H^{\circ} = 200 k J m o l^{- 1} Δ S^{\circ} = 40 J m o l^{- 1}$
The temperature at which equilibrium constant is unit is :

Calculate value of $^{'} l n (K_{e q})$ ' for the reaction at 250 K.
$N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)$
Given: $H_{f}^{0} ((N O_{2}) g) = + 40.407 k J / m o l$
$H_{f}^{0} ((N_{2} O_{4}) g) = + 70 k J / m o l$
$S_{r}^{0} = 10 J K^{- 1}$

At 473 K, $K_{c}$ for the reaction:
$P C l_{5 (g)} ⇌ P C l_{3 (g)} + C l_{2 (g)}$ is $8.3 \times 1 0^{- 3}$ .

What will be the value of $K_{c}$ , for the formation of $P C l_{5 (g)}$ at the same temperature?

$1$ mole of $N O$ and $1$ mole of $O_{3}$ are taken in a $10 L$ vessel and heated. At equilibrium, $50 %$ of $N O$ (by mass) reacts with $O_{3}$ according to the equation:

$N O_{(g)} + O_{3 (g)} ⇌ N O_{2 (g)} + O_{2 (g)}$

What will be the equilibrium constant for this reaction?

More topics

Relationship between Equilibrium Constant, Reaction Quotient and Gibbs Energy

Overview

Learn

Videos

Study Materials

Quick summary with Stories

Relation Between Gibbs Free Energy and Equillibrium Constant

Revise with Concepts

Relating Equilibrium Constant, Reaction Quotient and Gibbs Free Energy

Related questions

A vessel contains three gases A, B and C in the equilibrium: A⇌2B+C At equilibrium, the concentration of A was 3M and that of B was 4M. On doubling the volume of the vessel, the new equilibrium concentration of B was 3M. Calculate Kc​ and the initial equilibrium concentration of C.

A reaction mixture containing H2​,N2​ and NH3​ has partial pressure 2 atm, 1atm and 3 atm respectively at 725 K. If the value of K for the reaction. N2​+3H2​⇌2NH3​ is 4.28×10−5 atm−2 at 725 K, in which direction the net reaction will go:

△G∘ for 21​N2​+23​H2​⇌NH3​ is −16.5 kJ mol−1 at 25∘C. Find out Kp​ for the reaction. Also report Kp​ and △G∘ for: N2​+3H2​→2NH3​ at 25∘C.

The equilibrium constant of a reaction doubles on increasing the temperature of the reaction from 25oC to 35oC. Calculate enthalpy change of the reaction, assuming it to be constant in this temperature range.

Density of equilibrium mixture of N2​O and NO2​ at 1 atm and 384 K is 1.84 g/dm3. Equilibrium constant of the following reaction is: N2​O4​⇌2NO2​

1 mole of PCl3​ and 1 mole of PCl5​ is taken in a vessel of 10 L capacity maintained at 400 K.At equilibrium, the moles of Cl2​ is found to be 4×10−3

Steam undergoes decomposition at high temperature as per the reaction H2​O(g)⇌H2​(g)+21​O2​(g),ΔH∘=200kJmol−1ΔS∘=40Jmol−1 The temperature at which equilibrium constant is unit is :

Calculate value of ′ln(Keq​)' for the reaction at 250 K. N2​O4​(g)⇌2NO2​(g) Given: Hf0​((NO2​)g)=+40.407kJ/mol Hf0​((N2​O4​)g)=+70kJ/mol Sr0​=10JK−1

At 473 K, Kc​ for the reaction: PCl5(g)​⇌PCl3(g)​+Cl2(g)​ is 8.3×10−3. What will be the value of Kc​, for the formation of PCl5(g)​ at the same temperature?

1 mole of NO and 1 mole of O3​ are taken in a 10 L vessel and heated. At equilibrium, 50% of NO (by mass) reacts with O3​ according to the equation: NO(g)​+O3(g)​⇌NO2(g)​+O2(g)​ What will be the equilibrium constant for this reaction?

More topics

A reaction mixture containing $H_{2}, N_{2}$ and $N H_{3}$ has partial pressure 2 atm, 1atm and 3 atm respectively at 725 K. If the value of K for the reaction. $N_{2} + 3 H_{2} ⇌ 2 N H_{3}$ is $4.28 \times 1 0^{- 5}$
atm $^{- 2}$ at 725 K, in which direction the net reaction will go:

$△ G^{\circ}$ for $\frac{1}{2} N_{2} + \frac{3}{2} H_{2} ⇌ N H_{3}$ is $- 16.5 k J m o l^{- 1}$ at $2 5^{\circ} C$ . Find out $K_{p}$ for the reaction. Also report $K_{p}$ and $△ G^{\circ}$ for:

$N_{2} + 3 H_{2} \to 2 N H_{3}$ at $2 5^{\circ} C$ .

The equilibrium constant of a reaction doubles on increasing the temperature of the reaction from $2 5^{o} C$ to $3 5^{o} C$ . Calculate enthalpy change of the reaction, assuming it to be constant in this temperature range.

Density of equilibrium mixture of $N_{2} O$ and $N O_{2}$ at 1 atm and 384 K is $1.84 g / d m^{3}$ . Equilibrium constant of the following reaction is:
$N_{2} O_{4} ⇌ 2 N O_{2}$

1 mole of $P C l_{3}$ and 1 mole of $P C l_{5}$ is taken in a vessel of 10 L capacity maintained at 400 K.At equilibrium, the moles of $C l_{2}$ is found to be $4 \times 1 0^{- 3}$

Steam undergoes decomposition at high temperature as per the reaction
$H_{2} O (g) ⇌ H_{2} (g) + \frac{1}{2} O_{2} (g), Δ H^{\circ} = 200 k J m o l^{- 1} Δ S^{\circ} = 40 J m o l^{- 1}$
The temperature at which equilibrium constant is unit is :

Calculate value of $^{'} l n (K_{e q})$ ' for the reaction at 250 K.
$N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)$
Given: $H_{f}^{0} ((N O_{2}) g) = + 40.407 k J / m o l$
$H_{f}^{0} ((N_{2} O_{4}) g) = + 70 k J / m o l$
$S_{r}^{0} = 10 J K^{- 1}$

At 473 K, $K_{c}$ for the reaction:
$P C l_{5 (g)} ⇌ P C l_{3 (g)} + C l_{2 (g)}$ is $8.3 \times 1 0^{- 3}$ .

What will be the value of $K_{c}$ , for the formation of $P C l_{5 (g)}$ at the same temperature?

$1$ mole of $N O$ and $1$ mole of $O_{3}$ are taken in a $10 L$ vessel and heated. At equilibrium, $50 %$ of $N O$ (by mass) reacts with $O_{3}$ according to the equation:

$N O_{(g)} + O_{3 (g)} ⇌ N O_{2 (g)} + O_{2 (g)}$

What will be the equilibrium constant for this reaction?