One mole of an ideal diatomic gas $(C_V = 5 \ cal)$ was transformed from initial $25 \ ^{\circ}C$ and $1 \ L$ to the state when temperature is $100 \ ^{\circ}C$ and volume $10 \ L$. The entropy change of the process can be expressed as $(R = 2 \ cal / mol \cdot K)$ :-
- A$3 \ln \frac{298}{373} + 2 \ln 10$
- B$5 \ln \frac{373}{298} + 2 \ln 10$
- C$7 \ln \frac{373}{298} + 2 \ln \frac{1}{10}$
- D$5 \ln \frac{373}{298} + 2 \ln \frac{1}{10}$
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