One mole gas is first colled from `300 K` to `150 K` at constant volume and then heated from `150K` to `300 K` at constant pressure. The net heat absorbeed by the gas is

The temperature of 20 litres of nitrogen was increased from 100 K to 300 K at a constant pressure. Change in volume will be

The temperature of 20 litres of nitrogen was increased from 100 K to 300 K at a constant pressure. Change in volume will be

300 ml of a gas at 300 K is cooled to 276 K at constant pressure. The final volume is

300 ml of a gas at 300 K is cooled to 276 K at constant pressure. The final volume 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:

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 :-

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 :-

One mole of an ideal gas is heated from 300 K to 700 K at constant pressure. The change ininternal energy of the gas for this process is 8 kJ. What would be the change in enthalpy (in kJ) for the same process? ( R=8 " J"//"mole" -K )