At constant temperature and pressure same amount of air is adiabatically compressed to`1/4th` of its original volume. What will be the change, in temperature?

Some amount of air, initially at STP, is adiabatically compressed to 1/5 th its initial volume. Determine the rise in temperature. Given, gamma = 1.41 .

A monoatomic gas X and a diatomic gas Y, both initially at the same temperature and pressure are compressed adiabatically (separately) from a volume V to V/2, which gas will be at higher temperature?

By adiabatic compression the volume of a gas at 27^@C is reduced to to 8//27 of the initial volume. What is the change of its temperature?

If certain amount of gas is compressed suddenly and the pressure is increased by 8 times of its initial pressure, and gamma = 1.5 then what will be the change in temperature?

How will the temperature of an ideal gas change in an adiabatic compression?

A gas is kept in a closed containers at constant temperature. Keeping the temperature constant if some amount of the gas is incorporated.what will be the change in pressure?

(i) The pressure and temperature of 0.8 g of He gas are 1 atm and 298 K respectively. If 400 J of heat is applied to the gas at constant volume, what will be change in internal energy and the final temperature of the gas ? (ii) If the same amount of heat is applied to the gas at constant pressure, then what will be the change in internal energy and the final temperature of the gas ? For both the cases, assume He gas behaves ideally and its C_(V)=(3)/(2)R .

For an ideal gas, C_(V)=(3)/(2)R . (a) What will be the change in internal energy (DeltaU) of 1 mole of an ideal gas if its temperature is increased by 4K at constant volume ? What would be DeltaU if the temperature of this gas is increased by the same amount of constant pressure? keeping pressure constant if the temperature of that same amount of gas is increased by 4K then what will be the change in internal energy (DeltaU) of that gas? (c) give reason for different values of DeltaU and DeltaH ?