5 mole of ideal gas at `100K(C_(v.m)=28J//mol//K)`. It is heated upto 200 K. calculate `triangleU` and `triangle(PV)` for the process `(R=8J//mol-K)`

5 moles of an ideal gas at 100 K are allowed to undergo reversible compression till its temperature becomes 200 K If C_(V) = 28 J K^(-1)mol^(-1) , calculate DeltaU and DeltapV for this process. (R = 8.0 JK^(-1)mol^(-1) ]

1 mole of an ideal gas expands from 5 dm^(3) " to" 25 dm^(3) isothermally and irreversibly at 27^(@) C. Find work done in the process [R=8.3 J//mol//K ]

Three moles of an ideal gas (C_(v,m) = 12.5 J K^(-1) mol^(-1)) are at 300 K and 5 dm^(3) . If the gas is heated to 320K and the volume changed to 10 dm^(3) , calculate the entropy change.

Three moles of an ideal gas (C_(v,m) = 12.5 J K^(-1) mol^(-1)) are at 300 K and 5 dm^(3) . If the gas is heated to 320K and the volume changed to 10 dm^(3) , calculate the entropy change.

For an ideal gas C_(V,m)=12.47J*mol^(-1)*K^(-1) . What will be the value of C_(P,m) ?

Two moles of an ideal gas was heated isobarically so that its temperature was raised by 100 K. The heat absorbed during the process was 4000 J. Calculate (i) the work done by the gas, (ii) the increase in internal energy and (ii) the value of y for the gas [R =8.31 J mol ^(-1) K ^(-1) ].

Three moles of an ideal gas kept at a constant temperature of 300 K are compressed from a volume of 4 litre to 1 litre. Calculate the work done in the process. (R = 8.31 J mol^-1 K^-1 )