If `1 gram` of oxygen at `760 mm` pressure and `0^(@)C` has its volume double in an adiabatic change , calculate the change in internal energy. Take `R=2 cal. Mol e^(-1)K^(-1)= 4.2J cal^(-1) and gamma=1.4`.

Ten mole of hydrogen at N.T.P is compressed adiabatically so that it temperature becomes 400^(@)C . How much work is done on the gas? Also, Calculate the increase in internal energy of the gas. Take R=8.4J mol e^(-1)K^(-1) and gamma= 1.4 .

1 mole of an ideal gas at STP is subjected to a reversible adiabatic expansion to double its volume. Find the change in internal energy ( gamma = 1.4)

1 g mole of an ideal gas at STP is subjected to a reversible adiabatic expansion to double its volume. Find the change in internal energy ( gamma = 1.4)

A litre of hydrogen at 27^@C and 10^5 Nm^-2 pressure expand isothermally until its volume is doubled and then adiabatically until its volume is redoubled. Find the final pressure of the gas. 1(gamma = 1.4)

A gram molecule of gas at 27^(@)C expands isothermally untill its volume is doubled. Find the amount of work done and heat absorbed. Take R=8.31J mol e^(-1) K^(-1) .

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)]

The specific heat of argon at constant volume is 0.075 kcal kg^(-1) K^(-1) . Calculate its atomic weight. Take R = 2 cal mol^(-1) K^(-1) .

A gaseous system absorbs 450 cal heat. The work done by the system is 836.2 J. Find the change in internal energy of the gas in calorie. (J=4.186 J "cal"^(-1) )

A system absorbs 100 cal of heat and does an external work of 150 J. if J=4.2 J/cal the change in internal energy is