For the reaction H 2 ( g ) + Br 2 ( l ) → 2 H + ( aq ) + 2 Br − ( aq ) ; Δ G ∘ = − 207.4 kJ the Gibbs energy of formation Δ G f ∘ of Br − ( aq ) is:

H 2 ( g ) , Br 2 ( l ) and H + ( aq ) all have Δ G f ∘ = 0 . Δ G r x n ∘ = 2Δ G f ∘ ( Br − ) = − 207.4 . Δ G f ∘ ( Br − ) = − 103.7 kJ/mol . Answer: (A).

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ChemistryThermodynamics - IIGibb's Free EnergyMedium2 minQB

ChemistryMediumsingle choice

For the reaction

$H_{2} (g) + Br_{2} (l) \to 2 H^{+} (aq) + 2 Br^{-} (aq)$ ; $Δ G^{\circ} = - 207.4 kJ$

the Gibbs energy of formation $Δ G_{f}^{\circ}$ of $Br^{-} (aq)$ is:

Options:

Answer:

Solution:

$H_{2} (g)$ , $Br_{2} (l)$ and $H^{+} (aq)$ all have $Δ G_{f}^{\circ} = 0$ .

$Δ G_{r x n}^{\circ} = 2Δ G_{f}^{\circ} (Br^{-}) = - 207.4$ .

$Δ G_{f}^{\circ} (Br^{-}) = - 103.7 kJ/mol$ .

Answer: (A).

Stream:JEESubject:ChemistryTopic:Thermodynamics - IISubtopic:Gibb's Free Energy

⏱ 2mℹ️ Source: QB

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