Question

enthalpy and entropy changes of a reaction be reversed 40.53 Kj +108.8 Jk^-1 respectively. predict the feasibility of the reaction at 27 degree C.​

Answer 1

Given that

$\large\rm { \Delta H = 40.63 \frac{kJ}{mol}}$

$\large\rm { \Delta S = 108.8 \ Jk^{-1} }$

$\large\rm { T = (27+273) K}$

$\large\rm { T = 300 K}$

Now,

$\large\rm { \Delta G = \Delta H - T \Delta S}$

$\large\rm { = 40.63 \times 10^{3} - 300 \times 108.8}$

$\large\rm { = 40630-32640}$

$\large\rm { = 7,990}$

Hence, it is non-spotaneous.

Answer 2

Answer:

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