During adiabatic expansion,if the temperature | vedclass

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(A) For an adiabatic process,the first law of thermodynamics states that $Q = \Delta U + W$. Since the process is adiabatic,$Q = 0$,so $W = -\Delta U$

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$375$

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(A) For an adiabatic process,the first law of thermodynamics states that $Q = \Delta U + W$. Since the process is adiabatic,$Q = 0$,so $W = -\Delta U$.The change in internal energy is given by $\Delta U = n C_v \Delta T$.For a diatomic gas,the molar heat capacity at constant volume is $C_v = \frac{5}{2} R$.Given: $n = 3$ moles,$\Delta T = -50^{\circ} C$ (since temperature decreases).Therefore,$\Delta U = 3 	imes (\frac{5}{2} R) 	imes (-50) = 3 	imes 2.5 R 	imes (-50) = -375 R$.The work done by the gas is $W = -\Delta U = -(-375 R) = 375 R$.

During adiabatic expansion,if the temperature of $3$ moles of a diatomic gas decreases by $50^{\circ} C$,then the work done by the gas is (where $R$ is the Universal gas constant). (in $R$)

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