A) 1904 J
B) 2072 J
C) 2240 J
D) 2408 J
Correct Answer: B
Solution :
From first law of thermodynamics, we have \[{{k}_{1}}\] Which states that if an amount of heat Q is given to a system, a part of it will be used in increasing the internal energy \[{{F}_{1}}=-{{k}_{1}}{{y}_{1}}\] of the system and the rest in doing work (W). \[{{F}_{2}}=-{{k}_{2}}{{y}_{2}}\] We have \[{{k}_{2}}\] and \[{{k}_{1}}\] \[{{k}_{2}}{{F}_{1}}+{{k}_{1}}{{F}_{2}}=-{{k}_{1}}{{k}_{2}}({{y}_{1}}+{{y}_{2}})=-{{k}_{1}}{{k}_{2}}y\] \[{{F}_{1}}={{F}_{2}}=F(say)\] Note: Internal energy of a system is the energy possessed by the system due to molecular motion and molecular configuration. The energy due to molecular motion is called internal kinetic energy \[({{k}_{1}}+{{k}_{2}})F=-{{k}_{1}}{{k}_{2}}y\] and that due to molecular configuration is called internal potential energy \[{{U}_{p}}\]. It means \[\Rightarrow \]
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