An engine takes in 5 moles of air at `20^(@)C` and 1 atm, and compresses it adiabaticaly 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 ot be X kj. The value of X to the nearest interger 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

A gas expands against a constant pressure of 1 atm from a volume of 5L to 10L. During the process, system absorbs 400 J of heat from the surroundings. Calculate the change in the internal energy of the system.

In a container, two moles of a diatomic ideal gas is allowed to expand against 1 atm pressrue & volume change from 2 litre of 5 litre then calculate change in internal energy.

500cm^(3) of a sample of an ideal gas is compressed by an average pressure of 0.1 atm of 250 cm^(3) . During this process, 10J of heat flows out to the surroundings. Calculate the change in internal enegry of the system.

500cm^(3) of a sample of an ideal gas is compressed by an average pressure of 0.1 atm of 250 cm^(3) . During this process, 10J of heat flows out to the surroundings. Calculate the change in internal enegry of the system.

A diatomic gas which has initial volume of 10 liter is isothermally compressed to 1//15^(th) of its original volume where initial pressure is 10^(5) Pascal. If temperature is 27^(@)C then find the work done by gas

An ideal monoatomic gas initially in state 1 with pressure P_(1)=20 atm and volume V_(1)1500cm^(3) it is then taken to state 2 with pressure P_(2)=1.5P_(1) and volume V_(2)=2V_(1) find the change in internal energy in this process in KJ. (take 1atm lit =100J )

An ideal gas at pressure 2.5 xx 10^(5) pa and temperature 300k occupies 100 cc. It is adiabatically compressed to half its original volume. Calculate (a) the final pressure, (b) the final temperature and ( c) the work done by the gas in the process. Take (gamma = 1.5) .

At 27^(@)C two moles of an ideal monatomic gas occupy a volume. V The gas expands adiabatically to a volume 2V. Calculate (i) Final temperature of the gas (ii) change its internal energy and (iiI) Workd done by the gas during this process. Given R = 8.31 J//"mol" K, (2)^(2//3) = 1.587

A reversible heat engine carries 1 mole of an ideal monatomic gas around the cycle 1-2-3-1. Process 1-2 takes place at constant volume, process 2-3 is adiabatic, and process 3-1 takes place at constant pressure. Complete the values for the heat Delta Q , the change in internal energy Delta U , and the work done Delta , for each of the three processes and for the cycle as a whole.