When $2 \ mol$ of an ideal gas $\left( C_{p,m} = \frac{5}{2} R \right)$ is heated from $300 \ K$ to $600 \ K$ at constant pressure,the change in entropy of the gas $\left( \Delta S \right)$ is:
- A$\frac{3}{2} R \ln 2$
- B$-\frac{3}{2} R \ln 2$
- C$5 R \ln 2$
- D$\frac{5}{2} R \ln 2$
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View SolutionFor which of the following processes is the entropy change $(\Delta S)$ negative?
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$II)$ Freezing of water
$III)$ Crystallisation of the dissolved substance
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