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For a given reaction, $ΔH = 35 .5 {kJmol}^{- 1}$ and $ΔS = 83 .6 {JK}^{- 1} {mol}^{- 1}$ The reaction is spontaneous at(Assume that $ΔH and ΔS$ do not vary with temperature.)

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T > 425 K

all temperatures

T > 298 K

T < 425 K

answer is A.

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Detailed Solution

For a spontaneous reaction,

$ΔG < 0 i.e., ΔH - TΔS < 0 T > \frac{ΔH}{ΔS} T > (\frac{35.5 \times 1000}{83.6} = 424.6 \approx 425 K) ∴ T > 425 K$

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