Prove that the volume of a gas at `273^@C` is twice its volume at 273 K , at constant pressure.

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

Two moles of a gas at temperature T and volume V are heated to twice its volume at constant pressure. If (C _(p))/(C _(v)) = gamma then increase in internal energy of the gas is-

The temperature of a gas is increased by 1 °C. Then from the following statements pickout the correct one 1) The volume increases by 1/273 of its volume at 0°C at constant pressure 2) The pressure increases by 1/273 of its pressure at 0°C at constant volume 3) The volume decreases by 1/273 of its volume at 0°C 4) The pressure is doubled to its pressure at 0°C

The volume of a gas at 20^(@)C is 200 ml. If the temperature is reduced to -20^(@)C at constant pressure, its volume will be :-

At 18^@C , the volume occupied by the gas is 400 ml. To what temperature, it should be heated so that its volume gets doubled at constant pressure?

If V_(0) is the volume of a given mass of gas at 278 K at a constant pressure then according to Charle's law, the volume at 10^(@)C will be

Assertion : The pressure of a gas is inversely proportional to its volume at constant temperature and n. Reason : The gas volume is directly proportional to n at constant temperature and pressure .

The temperature of a given mass of a gas is increased from 19^(@)C to 20^(@)C at constant pressure. The volume V of the gas is

C_v and C_p denote the molar specific heat capacities of a gas at constant volume and constant pressure, respectively. Then

C_v and C_p denote the molar specific heat capacities of a gas at constant volume and constant pressure, respectively. Then