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. 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. 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) )

4.48 L of an ideal gas at STP requires 12 cal to raise the temperature by 15^(0)C at constant volume. The C_(P) of the gas is ____ cal