If Δ H=- text 25kcal, text T=300 text K and Δ S=9 text cal, then the reaction is

Question

If Δ H=- text 25kcal, text T=300 text K and Δ S=9 text cal, then the reaction is (A) spontaneous (B) non-spontaneous (C) equilibrium state (D) None of these

Tardigrade Admin · Accepted Answer

Δ G=Δ H-Δ .S ∵ Δ H=-25 kcal=-25000 cal T=300K, text Δ S=9cal Δ G=-25000-300× 9 =-25000-2700 Δ G=-27700 text cal The value of Δ G is negative, hence the reaction is spontaneous.

Q. If $Δ H = - 25 k c a l, T = 300 K$ and $Δ S = 9 c a l,$ then the reaction is

spontaneous

non-spontaneous

equilibrium state

None of these

$Δ G = Δ H - Δ. S$ $∵$ $Δ H = - 25 k c a l = - 25000 c a l$ $T = 300 K, Δ S = 9 c a l$ $Δ G = - 25000 - 300 \times 9$ $= - 25000 - 2700$ $Δ G = - 27700 c a l$ The value of $Δ G$ is negative, hence the reaction is spontaneous.

Q. If ΔH=−25kcal,T=300K and ΔS=9cal, then the reaction is