One mole of an ideal gas with `gamma=1.4` is adiabatically compressed so that its temperature rises from `27^(@)C` to `34^(@)C` . The change in the internal energy of the gas is `(R=8.3J mol^(-1)k^(-1))`

One mole of an ideal gas with gamma=1.4 is adiabatically compressed so that its temperature rises from 27^(@)C to 34^(@)C . The change in the internal energy of the gas is (R=8.3J mol^(-10k^(-1)))

One mole of an ideal gas (gamma=7//5) is adiabatically compressed so that its temperature rises from 27^(@)C to 35^(@)C the work done by the gas is (R=8.47J/mol-K)

One gm mol of a diatomic gas (gamma=1.4) is compressed adiabatically so that its temperature rises from 27^(@)C to 127^(@)C . The work done will be

Five moles of hydrogen (gamma = 7//5) , initially at STP , is compressed adiabatically so that its temperature becomes 400^(@)C . The increase in the internal energy of the gas in kilojules is (R = 8.30 J//mol-K)

5 moles of oxygen are heated at constant volume from 10^(@)C to 20^(@)C . The change in internal energy of a gas. [C_(P)=7.03 cal mol^(-1) deg^(-1) and R=8.3J mol^(-1) deg^(-1)]

A mass of diatomic gas (gamma=1.4) at a pressure of 2 atomphere is compressed adiabitically so that its temperature rises from 27^(@)C to 927^(@)C . The pressure of the gas in the final state is

One mole of a gas absorbs 200 J of heat at constant volume. Its temperature rises from 298 K to 308 K. The change in internal energy is :-