In which of the following reactions, standard entropy change ( Δ S ∘ ) is positive and standard Gibb's energy change ( Δ G ∘ ) decreases sharply with increasing temperature?

Since, in the first reaction gaseous products are forming from solid carbon hence entropy will increase i.e. Δ S = + ve . C ( gr . ) + 2 1 O 2 ( g ) → CO ( g ) ; Δ S ∘ = + ve Since, Δ G ∘ = Δ H ∘ − T Δ S hence the value of Δ G decrease on increasing temperature.

Chemistry - Thermodynamics - II Question with Solution | TestHub

ChemistryThermodynamics - IIRandomness and Third law of TDMedium2 minPYQ_2012

ChemistryMediumsingle choice

In which of the following reactions, standard entropy change $(Δ S^{\circ})$ is positive and standard Gibb's energy change $(Δ G^{\circ})$ decreases sharply with increasing temperature?

Options:

Answer:

Solution:

Since, in the first reaction gaseous products are forming from solid carbon hence entropy will increase i.e. $Δ S = + ve$ . $C (gr .) + \frac{1}{2} O_{2} (g) \to CO (g); Δ S^{\circ} = + ve$ Since, $Δ G^{\circ} = Δ H^{\circ} - T Δ S$ hence the value of $Δ$ G decrease on increasing temperature.

Stream:BITSATSubject:ChemistryTopic:Thermodynamics - IISubtopic:Randomness and Third law of TD

⏱ 2mℹ️ Source: PYQ_2012

Doubts & Discussion

Loading discussions...