2 mole of an ideal monoatomic gas undergoes a reversible process for which `PV^(2)=C`. The gas is expanded from initial volume of 1 L to final volume of 3 L starting from initial temperature of 300 K. Find `DeltaH` for the process :
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))]
1 mole of an ideal diatomic gas undergoes a reversible polytropic process (PV^(2)="constant") . The gas expand from initial volume of 1 litre and temp 300 K to final volume 3 lit. Claculate change in internal energy (approx).
1 mole of an ideal gas A(C_(v.m)=3R) and 2 mole of an ideal gas B are ((C_(v,m)=(3)/(2)R) taken in a container and expanded reversible and adiabatically from 1 litre of 4 letre starting from initial temperature of 320 K. DeltaE or DeltaU for the process is :
One mole of an ideal monoatomic gas at 1 atm, 300 K undergo a process in which pressure of gas is 8 atm then calculate W (in cal).
One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from initial volume of 1L to a state where its final pressure becomes equal to external pressure. If initial temperature of gas is 300K then total entropy change of system in the above process is: [R=0.082L atm mol^(-1) K^(-1)-=8.3J mol^(-1) K^(-1)]
What will be the entropy change when two moles of an ideal gas expand reversibly from initial volume of 1 litre to 10 litre at constant temperature of 300 K?
Calculate the entropy change when 1mole of an ideal gas expands reversibly form an initial volume of 2 L to a final voluume of 20L at 25^(@)C .
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
