Test Index

Thermodynamics

Section: Chemistry

Question : 34 of 34

Marks: +1, -0

300\ \text{K}

A \rightarrow P

\Delta S_{\text{sys}}

5\ \text{JK}^{-1}\ \text{mol}^{-1}

\text{kJ}\ \text{mol}^{-1}

Solution:

Given for the reaction

A \rightarrow P

Temperature

T=300\ \text{K}

Entropy change

\Delta S_{\;\text{system }} = 5\ \text{J}/\text{K}/\text{mol}

The heat absorbed by the system can be calculated using the formula:

\Delta H_{\;\text{system }} = T \times \Delta S_{\;\text{system }}

Substitute the given values:

\Delta H_{\;\text{system }} = 300\ \text{K} \times 5\ \text{J}/\text{K}/\text{mol} = 1500\ \text{J}/\text{mol}

Since the answer is needed in kilojoules per mole, convert joules to kilojoules:

1500\ \text{J}/\text{mol} = 1.5\ \text{kJ}/\text{mol}

Thus, the heat absorbed by the system is

1.5\ \text{kJ}/\text{mol}

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