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Strike441 [17]
3 years ago
9

For the decomposition of calcium carbonate, consider the following thermodynamic data (Due to variations in thermodynamic values

for different sources, be sure to use the given values in calculating your answer.): ΔH∘rxn 178.5kJ/mol ΔS∘rxn 161.0J/(mol⋅K) Calculate the temperature in kelvins above which this reaction is spontaneous.
Chemistry
1 answer:
In-s [12.5K]3 years ago
7 0

Answer : The temperature in kelvins is, T>1108.695K

Explanation : Given,

\Delta H = 178.5 KJ/mole = 178500 J/mole

\Delta S = 161.0 J/mole.K

Gibbs–Helmholtz equation is :

\Delta G=\Delta H-T\Delta S

As per question the reaction is spontaneous that means the value of \Delta G is negative or we can say that the value of \Delta G is less than zero.

\Delta

The above expression will be:

0>\Delta H-T\Delta S

T\Delta S>\Delta H

T>\frac{\Delta H}{\Delta S}

Now put all the given values in this expression, we get :

T>\frac{178500J/mole}{161.0J/mole.K}

T>1108.695K

Therefore, the temperature in kelvins is, T>1108.695K

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