An engine takes in 5 moles of air at `20^(@)C` and 1 atm, and compresses it adiabatically to `1//10^(th)` of the original volume. Assuming air to be a diatomic ideal gas made up of rigid molecules, the change in its internal energy during this process comes out to be X kJ. The value of X to the nearest integer is ________.

A diesel engine takes in 1 mole of air at 300 K, 1 atm pressure and compresses it adiabatically to (1)/(32)th of the original volume. Considering air as a diatomic ideal gas, the change in temperature is

The temperature of 3.00 mo! of an ideal diatomic gas is increased by 40.0^@C without changing the pressure of the gas. The molecules in the gas rotate but do not oscillate. If the ratio of change in internal energy of the gas to the amount of workdone by the gas is x/10 . Then the value of x (round off to the nearest integer is ________. (Given R = 8.31 J mol^(-1) K^(-1) )

The temperature of 3.00 mo! of an ideal diatomic gas is increased by 40.0^@C without changing the pressure of the gas. The molecules in the gas rotate but do not oscillate. If the ratio of change in internal energy of the gas to the amount of workdone by the gas is x/10 . Then the value of x (round off to the nearest integer is ________. (Given R = 8.31 J mol^(-1) K^(-1) )

Work done on a system when one mole of an an ideal gas at 500 K is compressed isothermally and reversibly to 1/10th of its original volume. (R = 2cal)

At 27^@C two moles of an ideal monoatomic gas occupy a volume V. The gas expands adiabatically to a volume 2V. Calculate (i) the final temperature of the gas, (ii) change in its internal enegy, and (iii) the work done by the gas during this process.

How much work is done on the steam when 1.00 mol of water at 100^(@)C boils and becomes 1.00 mole of steam at 100^(@)C at 1.00 atm pressure? Assume the steam to behave as an ideal gas , detemine the change in the internal energy of the material as it vapourizes.

A mass of ideal gas at pressure P is expanded isothermally to four times the original volume and then slowly compressed adiabatically to its original volume. Assuming gamma to be 1.5, the new pressure of the gas is

An ideal gas at initial temperature 300 K is compressed adiabatically ( gamma = 1.4 ) to (1/16)^(th) of its initial volume. The gas is then expanded isobarically to double its volume. Then final temperature of gas round to nearest integer is:

At 27^@C two moles of an ideal monatomic gas occupy a volume V. The gas expands adiabatically to a volume 2V . Calculate (a) final temperature of the gas (b) change in its internal energy and (c) the work done by the gas during the process. [ R=8.31J//mol-K ]

An ideal gas in a cylinder is slowly compressed to one third of its original volume. During this process, the temperature of the gas remains constant and the work done in compression is 75 J. How much does the internal energy of the gas change ?