Five moles of hydrogen `(gamma = 7//5)`, initially at `STP`, is compressed adiabatically so that its temperature becomes `400^(@)C`. The increase in the internal energy of the gas in kilojules is `(R = 8.30 J//mol-K)`

5 moles of Hydrogen (gamma =(7)/(5)) initially at STP are compressed adiabatically so that its temperature becomes 400^(@)C . The increase in the internal energy of the gas in kilo-joule is [R =8.30 J mol^(-1)K^(-1)]

Five moles of hydrogen initially at STP is compressed adiabatically so that its temperature becomes 673 K. The increase in internal energy of the gas , in kilo joule is (R= 8.3 J // mol-K, gamma = 1.4 for diatomic gas)

Five moles of hydrogen initially at STP is compressed adiabatically so that its temperature becomes 673K. The increase in internal energy of the gas, in kilo joule is (R=8.3J/molK, gamma =1.4 for diatomic gas)

Ten mole of hydrogen at N.T.P is compressed adiabatically so that it temperature becomes 400^(@)C . How much work is done on the gas? Also, Calculate the increase in internal energy of the gas. Take R=8.4J mol e^(-1)K^(-1) and gamma= 1.4 .

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 with gamma = 1.4 , is adiabatically compressed so that its temperature rises from 42°C to 48°C . The change in the internal energy of the gas is ( R = 8.3 J / mol / K )

300K a gas (gamma = 5//3) is compressed adiabatically so that its pressure becomes 1//8 of the original pressure. The final temperature of the gas is :