A sample of ideal gas `(gamma = 1.4)` is heated at constant pressure. If an amount of 140 J of heat is supplied to the gas, find change in internal energy of the gas.

A sample of ideal gas (gamma = 1.4) is heated at constant pressure. If an amount of 140 J of heat is supplied to the gas, find work done by the gas.

A certain volume of a gas expands at one standard atmosphere pressure when 400 cal of heat is supplied to it. If there is no change in the internal energy of the gas, calculate its volume expansion.

A monatomic ideal gas is heated at constant pressure. How much fraction of heat is used to increase internal energy?

An ideal mono-atomic gas of given mass is heated at constant pressure. In this process, the fraction of supplied heat energy used for the increase of the internal energy of the gas is

The change in internal energy of an ideal gas becomes zero

One mole of an ideal monatomic gas is heated at a constant pressure from 0^(@)C to 100^(@)C . Then the change in the internal energy of the gas is (given R = 8.32 J cdot mol cdot k^(-1))

A gas confined in a cylinder with a frictionless piston is made to expand from 1L to 5L under constant pressure of 1.5 atm. During the process, 800J of heat is supplied from external source. Calculate the change in internal energy off the gas. (1L*atm=101.3J) .

(i) The pressure and temperature of 0.8 g of He gas are 1 atm and 298 K respectively. If 400 J of heat is applied to the gas at constant volume, what will be change in internal energy and the final temperature of the gas ? (ii) If the same amount of heat is applied to the gas at constant pressure, then what will be the change in internal energy and the final temperature of the gas ? For both the cases, assume He gas behaves ideally and its C_(V)=(3)/(2)R .