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A reaction has a value of, ∆H= -20Kcal at 200K, the reaction is spontaneous, below this temperature, it is not. The values ∆G and ∆S at 400K are respectively?

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10Kcal, -0.1cal

K^{- 1}

-10Kcal, -100cal

K^{- 1}

0 Kcal, -10.0cal

K^{- 1}

20 Kcal, -100cal

K^{- 1}

answer is D.

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Detailed Solution

ΔG = ΔH - TΔS

{0 = ΔH - TΔS}_{}

ΔH = TΔS

{- 20000 = (200) S}_{}

{S = \frac{- 20000}{200} = 100 cal / K}_{}

{S = 0.1 Kcal / K}_{}

Let’s find out the Gibbs free energy at 400K
At, 400K

ΔG = (- 20 + 4000 \times {0.1) Kcal}_{}

ΔG = 20 Kcal

So,

ΔG = 20 Kcal and S = - 100 cal / K or 0.1 {Kcal / K}_{}

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