[" 5One mole of an ideal diatomic gas "(C_(v)=5" cal) was transformed from initial "25C" and "1L" to the state "],[" when temperature is "100C" and volume "10L" .The entropy change of the process can be expressed as "],[(R=2" calories "/mol/K):-]

One mole of an ideal diatomic gas (C_(v) =5 cal) was transformed from initial 25^(@) and 1 L to the state when temperature is 100^(@) C and volume 10 L. The entropy change of the process can be expressed as ( R=2 calories /mol/K)

One mole of an ideal diatomic gas (C_(v)=5cal) was transformed form initial 25^(@)C and 1L to the state when the temperature is 100^(@)C and volume 10L. The entropy change of the process can be express as: (R=2cal//mol//K)

One mole of an ideal diatomic gas (C_(v)=5cal) was transformed form initial 25^(@)C and 1L to the state when the temperature is 100^(@)C and volume 10L. The entropy change of the process can be express as: (R=2cal//mol//K)

One mole of an ideal diatomic gas (C_(v) =5 cal) was transformed from initial 25^(@) and 1 L to the state when temperature is 100^(@) C and volume 10 L. Then for this process(R= 2 "calories" //"mol"//K" )(take calories as unit of energy and kelvin for temp)

One mole of an ideal diatomic gas (C_(v)=5 cal K^(-1) "mole"^(-1)) chagre its state from state 1 (27^(@) C 1 L) to state 2 (127^(@) C, 10L) . For this process, which of the following is (are) correct? (Given : R=2 cal K^(-1) "mole"^(-1))

One mole of an ideal gas expands isothermally from 10 L to 100 L. Change in entropy of the process will be

1 mole of an ideal diatomic gas undergoes a reversible polytropic process (PV^(2)=K) .The gas expands from initial volume of 1L to 3L and initial temperature of 300K what is the change in internal energy |Delta U| in cal [(R=2calmol^(-1)K^(-1))]

One mole of an ideal gas at 300 K is expanded isothermally from an initial volume of 1 L to 10 L. The DeltaE for this process is (R=2 cal . "mol"^(-1)K^(-1) )