By Opening The Door Of A Refrigerator Inside A Closed Room:

An ideal gas is taken through a cyclic thermo-dynamical process through four steps. The amounts of heat involved in these steps are:

    respectively. The corresponding works involved are:  respectively. The value of W₄ is:

When an ideal diatomic gas is heated at constant pressure fraction of the heat energy supplied which increases the internal energy of the gas is:

70 calories of heat are required to raise the temperature of 2 moles of an ideal gas at constant pressure from 30^oC to 35^oC. The amount of heat required to raise the temperature of the same gas through same range (30^oC to 35^oC) at constant volume is:

A motor-car tyre has a pressure of 2 atmosphere at 27^oC. It suddenly bursts. If (C_p/C_v) = 1.4 for air, find the resulting temperature:

Find the  amount of work done to increase the  temperature of one mole of ideal gas by 30^oC, if it is expanding under the condition  (R = 8.31 J/mol-K):

For an adiabatic expansion of a perfect gas, the value of  is equal to:

In an adiabatic expansion of a gas, the product of pressure and volume:

One of the most efficient engines ever developed operates between 2100 K and 700 K. Its actual efficiency is 40%. What percentage of its maximum possible efficiency is this?

In an adiabatic change, the pressure P and temperature T  of a diatomic gas are related by the relation   where C equals:

One mole of an ideal mono-atomic gas is heated at a constant pressure of one atmosphere from 0^oC to 100^oC. Then the change in the internal energy is: