What is the change internal energy when a gas contracts from 377 mL to 177 mL under a constant pressure of 1520 torr, while at the same time being cooled by removing 124 J heat ? `[Take :( 1 L atm ) =100 J)]`
6 what is the change in internal energy when a gas contracts from 377 ml to 177 ml under a constant pressure of 1520 torr, while at the same time being cooled by removing 124 J heat? [Take (1 L atm)= 100J]
A gas can expand from 100 ml to 250 ml under a constant pressure of 2 atm. The work done by the gas is
An ideal gas is heated from 20^(@)C to 40^(@)C under constant pressure. The change in internal energy is
An office room contains about 2000 moles of air . The change in the internal energy of this much air when it is cooled from 34 ^@ C to 24^@C at constant pressure of 1.0 atm is [ Use gamm _(" air") = 1.4 and universal gas constant =8.314 J // mol -K]
The internal energy of an ideal gas is given by U = 1.5 PV. It expands from 10 cm^(3) to 20 cm^(3) against a constant pressure of 2 xx 10^(5) Pa. heat absorbed by the gas in the process is
A gas absorbs 100 calories of heat energy and is compressed from 10L to 5L by applying an external pressure of 2 atm. Change in internal energy in calories will be nearly.
Find the change in internal energy in joule when 20gm of a gas is heated from 20^(@)C to 30^(@)C (G = 0.18 kcal/kg K, J = 4200J/kcal)
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
