One gm mole of an ideal gas at S.T.p is subjected to a reversible adiabatic expansion to double its. volume Find the change in internal energy in the process. Given `=gamma=1.4`.

1 mole of an ideal gas at 25^@C is subjected to expand reversibly ten times of its intial volume. The change in entropy of expansion is:

A certain mass of gas is allowed to expand adiabatically to 6 times its original volume. Find the relation between the initial and final pressure. gamma=1.4 .

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:

Two identical samples of gas are allowed to expand to double it’s volume, one adiabatically and the other isothermally. In which case more work is done ?

10 moles of hydrogen at N.T.p is compressed adiabatically so that its temperature becomes 400^@C . How much work in Joule is done on the gas ? What is the increase in internal energy of the gas. Given R=8.31"jmole"^-1k^-1 and gamma=1.4 .

One mole of an ideal gas expands adiabatically from temperature T_1 to T_2 .the workdone by the gas is_____.

One gram mole of oxygen gas at 127^@C expands isothermally until its volume is doubled. Find the amount of work done and heat produced R=8.314"jmole"^-1k^-1

One gm of water at 373 K is converted into steam at the same temperature. The volume of 1 c .c of water becomes' 1671 c.c on boiling. Calculate the change in internal energy of the system if heat of vaporisation of water is 5.4xx10^5calkg^-1 .

An ideal gas at 27^@C and a pressure of760 mm of mercury is compressed isotiiermally until its volume is halved. It is then expanded adiabatically to twice its original volume. If the value of gamma for the gas is 1.4. Calculate the final pressure and temperature of the gas.