In conversion of lime-stone to lime, CaCO 3 ( s ) ⟶ CaO ( s ) + CO 2 ( g ) the vales of Δ H ∘ and Δ S ∘ are + 179.1 kJ mol − 1 and 160.2 J / K respectively at 298 K and 1 bar . Assuming that Δ H ∘

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In conversion of lime-stone to lime, CaCO 3 ​ ( s ) ⟶ CaO ( s ) + CO 2 ​ ( g ) the vales of Δ H ∘ and Δ S ∘ are + 179.1 kJ mol − 1 and 160.2 J / K respectively at 298 K and 1 bar . Assuming that Δ H ∘ do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is

TestHub · Accepted Answer

We know, Δ G = Δ H − T Δ S So, lets find the equilibrium temperature, i.e. at which ​ Δ G = 0 Δ H = T Δ S T = 160.2 179.1 × 1000 ​ = 1118 K ​ So, at temperature above this, the reaction will become spontaneous. Hence, (D) is correct answer.

Chemistry - Thermodynamics - II Question with Solution | TestHub

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