2 mole of an ideal gas at $$ 27^{\circ} \mathrm{C} $$ temperature is expanded reversibly from 2 lit to 20 lit. Find the entropy change. $$ (R=2 \mathrm{cal} / \mathrm{mol} \mathrm{K}) $$ $$ \begin{array}{llll} ext { (a) } 92.1 & ext { (b) } 0 & ext { (c) } 4 & ext { (d) }-9.2\end{array} $$

Question

2 mole of an ideal gas at $$ 27^{\circ} \mathrm{C} $$ temperature is expanded reversibly from 2 lit to 20 lit. Find the entropy change. $$ (R=2 \mathrm{cal} / \mathrm{mol} \mathrm{K}) $$ $$ \begin{array}{llll}	ext { (a) } 92.1 & 	ext { (b) } 0 & 	ext { (c) } 4 & 	ext { (d) }-9.2\end{array} $$

Patel Guzman · Accepted Answer

The entropy change is approximately 9.21 cal/K.

2 mole of an ideal gas at \( 27^{\circ} \mathrm{C} \) temperature is expanded reversibly from 2 lit to 20 lit. Find the entropy change. \( (R=2 \mathrm{cal} / \mathrm{mol} \mathrm{K}) \) \( \begin{array}{llll}\text { (a) } 92.1 & \text { (b) } 0 & \text { (c) } 4 & \text { (d) }-9.2\end{array} \)

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2 mole of an ideal gas at \( 27^{\circ} \mathrm{C} \) temperature is expanded reversibly from 2 lit to 20 lit. Find the entropy change. \( (R=2 \mathrm{cal} / \mathrm{mol} \mathrm{K}) \) \( \begin{array}{llll}\text { (a) } 92.1 & \text { (b) } 0 & \text { (c) } 4 & \text { (d) }-9.2\end{array} \)

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