One mole of hydrogen, assumed to be ideal, is adiabatically expanded from its initial state $(P_{1}, V_{1}, T_{1})$ to the final state $(P_{2}, V_{2}, T_{2})$ . The decreases in the internal energy of the gas during this process will be given by

C_{v} (T_{1} - T_{2})

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C_{p} (T_{1} - T_{2})

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\frac{C_{P} + C_{V}}{2} (T_{1} - T_{2})

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(C_{p} - C_{v}) (T_{1} - T_{2})

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Solution

The correct option is C $C_{v} (T_{1} - T_{2})$
The change in the internal energy $= C_{v} Δ T$ .
Since $Δ T$ is positive there is an increase in internal energy given by $d U = C_{v} (T_{2} - T_{1})$ .
Hence, decrease in internal energy $= - d U$ .

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One mole of hydrogen, assumed to be ideal, is adiabatically expanded from its initial state (P1,V1,T1) to the final state (P2,V2,T2). The decreases in the internal energy of the gas during this process will be given by

The correct option is C Cv(T1−T2)The change in the internal energy =CvΔT.Since ΔT is positive there is an increase in internal energy given by dU=Cv(T2−T1). Hence, decrease in internal energy =−dU.

One mole of hydrogen, assumed to be ideal, is adiabatically expanded from its initial state $(P_{1}, V_{1}, T_{1})$ to the final state $(P_{2}, V_{2}, T_{2})$ . The decreases in the internal energy of the gas during this process will be given by

The correct option is C $C_{v} (T_{1} - T_{2})$
The change in the internal energy $= C_{v} Δ T$ .
Since $Δ T$ is positive there is an increase in internal energy given by $d U = C_{v} (T_{2} - T_{1})$ .
Hence, decrease in internal energy $= - d U$ .