The work of 146 kJ is performed in order to compress one k mole of a gas adiabatically and in this process the temperature of the gas increases by `7^(@)C`. Prove that the gas is diatomic. `R = 8.3 J cdot mol^(-1) cdot K^(-1)`.

What amount of heat is to be supplied to 14 g of nitrogen in order to increase the temperature by 40^(@)C at constant pressure? Molecular weight of nitrogen =28 and R = 8.3 J cdot mol^(-1) cdot K^(-1) .

10 mol of an ideal gas is taken through an isothermal process in which the volume is compressed from 40 L to 30 L. If the temperature and the pressure of the gas are 0^(@)C and 1 atm respectively. Find the work done in the process. Given: R = 8.31 J cdot mol^(-1) cdot K^(-1) .

70 cal of heat is required to increase the temperature of 2 mol of an ideal diatomic gas at constant pressure from 40^(@)C to 45^(@)C . How much heat will be required to increase the temperature of that gas by the same amount at constant volume? R = 2 cal cdot mol^(-1) cdot K^(-1) .

1 mol oxygen is kept in an insulated closed vessel. The vessel is suddenly moved at constant velocity v_(0) causing the temperature of the gas to rise by 1^(@)C . Find out the value of v_(0) . For oxygen , gamma = 1.41 and molar gas constant, R = 8.31 J cdot mol^(-1) cdot K^(-1) .

One mole of an ideal monatomic gas is heated at a constant pressure from 0^(@)C to 100^(@)C . Then the change in the internal energy of the gas is (given R = 8.32 J cdot mol cdot k^(-1))

Find out the molar specific heats C_(p) an C_(v) of an ideal gas having gamma = 1.67 . Given, R = 2 cal cdot mol^(-1) cdot^(@)C^(-1) .

What amount of heat must be supplied to 2.0 xx 10^(-2) kg of nitrogen (at room temperature) to raise its temperature by 45^(@)C at constant pressure? (Molecular mass of N_(2) = 28, R = 8.3 J cdot mol^(-1) cdot K^(-1))