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Relationship between equilibrium constant K, reaction quotient q and gibbs energy G

The following reaction is performed at 298 {~K}. 2 {NO}({g})+{

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Solving time: 4 mins

The following reaction is performed at $298 K$ .
$2 NO (g) + O_{2} (g) ⇌ 2 NO_{2} (g)$
The standard free energy of formation of $NO (g)$ is $86.6 kJ / mol$ at $298 K$ . What is the standard free energy of formation of $NO_{2} (g)$ at $298 K$ ? $(K_{p} = 1.6 \times 1 0^{12}$ )

86600 - \frac{ln ( 1.6 \times 1 0 ^{12} )}{R ( 298 )}

0.5 [2 \times 86, 600 - R (298) ln (1.6 \times 1 0^{12})]

R (298) ln (1.6 \times 1 0^{12}) - 86600

86600 + R (298) ln (1.6 \times 1 0^{12})

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Updated on: Dec 13, 2022

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The following reaction is performed at

298 K

2 NO (g) + O_{2} (g) ⇌ 2 NO_{2} (g)

The standard free energy of formation of

NO (g)

86.6 kJ / mol

298 K

. What is the standard free energy of formation of

NO_{2} (g)

298 K

(K_{p} = 1.6 \times 1 0^{12}

)

12 mins ago

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12 mins ago

Text solutionVerified

Δ G_{reaction}^{\circ} = 2Δ G_{f}^{\circ} (NO_{2}) - 2Δ G_{f}^{\circ} (NO) - Δ G_{f}^{\circ} (O_{2})

2Δ G_{f}^{\circ} (NO_{2}) = Δ G_{rex^{\circ}}^{\circ} + 2Δ G_{f}^{\circ} (NO) + Δ G_{f}^{\circ} (O_{2}) Δ G = Δ G^{\circ} + RT ln K_{p}

At equilibrium,

Δ G = 0, Q = K_{p}; Δ G^{\circ} = - RT ln K_{p}

Δ G_{f}^{\circ} (O_{2}) = 0

∴ Δ G_{f}^{\circ} (NO_{2}) = \frac{1}{2} [2 \times 86600 - R (298) ln (1.6 \times 1 0^{12})]

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Question Text	The following reaction is performed at $298 K$ . $2 NO (g) + O_{2} (g) ⇌ 2 NO_{2} (g)$ The standard free energy of formation of $NO (g)$ is $86.6 kJ / mol$ at $298 K$ . What is the standard free energy of formation of $NO_{2} (g)$ at $298 K$ ? $(K_{p} = 1.6 \times 1 0^{12}$ )
Updated On	Dec 13, 2022
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 3
Upvotes	322
Avg. Video Duration	4 min

The following reaction is performed at $298 K$ .
$2 NO (g) + O_{2} (g) ⇌ 2 NO_{2} (g)$
The standard free energy of formation of $NO (g)$ is $86.6 kJ / mol$ at $298 K$ . What is the standard free energy of formation of $NO_{2} (g)$ at $298 K$ ? $(K_{p} = 1.6 \times 1 0^{12}$ )

Text solutionVerified

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The following reaction is performed at 298 K. 2NO(g)+O2​( g)⇌2NO2​( g)The standard free energy of formation of NO(g) is 86.6 kJ/mol at 298 K. What is the standard free energy of formation of NO2​( g) at 298 K ? (Kp​=1.6×1012 )

Text solutionVerified

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The following reaction is performed at $298 K$ .
$2 NO (g) + O_{2} (g) ⇌ 2 NO_{2} (g)$
The standard free energy of formation of $NO (g)$ is $86.6 kJ / mol$ at $298 K$ . What is the standard free energy of formation of $NO_{2} (g)$ at $298 K$ ? $(K_{p} = 1.6 \times 1 0^{12}$ )