For a given reaction, =35.5kJ mol^ -1 and =83.6Jk^ -1 mol^ -1 . T… - Vidyadip

MCQ

For a given reaction, $\Delta\text{H}=35.5\text{kJ mol}^{-1}$ and $\Delta\text{S}=83.6\text{Jk}^{-1}\text{mol}^{-1}.$ The reaction is spontaneous at $($assume that $\Delta\text{H}$ and $\Delta\text{S}$ do not vary with temperature$)$

A
$T > 425K$
✓
All temperature
C
$T > 298K$
D
$T < 425K$

✓

Answer

Correct option: B.

All temperature

$\Delta\text{G}=\Delta\text{H}-\text{T}\Delta\text{S}$
$=0=35.5\times1000\text{J}-\text{T}\times83.6\text{Jk}^{-1}\text{mol}^{-1}$
$\Rightarrow\text{T}=\frac{35500}{83.6}=425\text{K}$
Above $425K, \Delta\text{G}=-\text{ve},$ therefore process will be spontaneous above $425K.$

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