If 5 moles of oxygen at STP is adiabatically compressed so that temperature increases to `400^@C`, then find the work done on the gas. R=8.3J/mole−K

5.6 liter of helium gas at STP is adiabatically compressed to 0.7 liter. Taking the initial temperature to be T_1, the work done in the process is

The work of 146 kJ is performed in order to compress one kilo mole of a gas adiabatically and in this process the temperature of the gas increases by 7^@C . The gas is (R=8.3ml^-1Jmol^-1K^-1)

One mole of an ideal gas is heated at constant pressure of 1 atmosphere form 0^@C to 100^@C the change in the internal energy is (R = 8 J/ mol K )

A cylinder containing one gram molecule of the gas compressed adiabatic ally until its temperature from 27^@C to 97^@C . Calculate the work done and heat produced in the gas. (y = 1.5)

In an isothermal reversible expansion, if the volume of 96 gm of oxygen at 27^(@)C is increased from 70 litres to 140 litres , then the work done by the gas will be

The specific heat of a gas at constant volume is 20J/mol ^@K . When two moles of such gas is heated through 10^@C at constant pressure, what is the increase in internal energy and work done ? (R= 8J/mol ^@ K)

Three moles of an ideal gas kept at a constant temperature of 300 K are compressed from a volume of 4 litre to 1 litre. Calculate the work done in the process. (R = 8.31 J mol^-1 K^-1 )

One mole of an ideal gas requires 135 J of heat to raise its temperature by 15 ^@ K when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same, then the heat required will be (R = 8.3J /mole ^@K)

One mole of an ideal gas at an initial temperature true of TK does 6R joule of work adiabatically. If the ratio of specific heats of this gas at constant pressure and at constant volume is 5//3 , the final temperature of the gas will be