From first law of thermodynamics Q=∆U+W For cylinder A pressure remains constant ∴ Work done by a system W=‌
µR
γ−1
(T1−T2) For monoatomic gases ‌µ‌=1 ∴‌=‌
5
3
∴‌=‌
1×R
5
3
−1
(442−400) ‌=‌
3
2
R×42 ‌‌ or ‌‌‌W‌=63R ‌‌ But ‌∆U=0,‌ for cylinder ‌A ∴‌Q‌=0+63R ‌Q‌=63R For cylinder B volume is constant, ∴‌‌W=0 and ‌‌Q=µCV∆T For monoatomic gas CV=‌
3
2
R Q=1×‌
3
2
R∆T As heat given to both cylinder is same ∴‌‌63R‌=‌