2 mol of CO was in the small cubical container of length, l=′a′ at 57 ∘C. The Gas was taken out completely from the small container and put into large container (l=′2a′) at the same temperature. What is the change in entropy, if it is assumed that the process is reversible and gas is behaving as an ideal one? (Take ln2=0.7, ln3=1.1, R=253J mol−1 K−1

2 mol of CO was in the small cubical container of length, l=′a′ at

1.	2 mol of CO was in the small cubical container of length, l=′a′ at 57 ∘C. The Gas was taken out completely from the small container and put into large container (l=′2a′) at the same temperature. What is the change in entropy, if it is assumed that the process is reversible and gas is behaving as an ideal one? (Take ln2=0.7, ln3=1.1, R=253J mol−1 K−1
Answer» 2 mol of $C O$ was in the small cubical container of length, $l =^{'} a^{'}$ at $57^{\circ} C$ . The Gas was taken out completely from the small container and put into large container $(l =^{'} 2 a^{'})$ at the same temperature. What is the change in entropy, if it is assumed that the process is reversible and gas is behaving as an ideal one? (Take $l n 2 = 0.7, l n 3 = 1.1, R = \frac{25}{3} J m o l^{- 1} K^{- 1}$