The temperature of the mixture of one mole of helium and one mole of hydrogen is increased from `0^(@)C` to `100^(@)C` at constant pressure. The amount of heat delivered will be

Five moles of hydrogen gas are heated from 30^(@)C to 60^(@)C at constant pressure. Heat given to the gas is (given R = 2 cal//mol degrees)

Five moles of hydrogen gas are heated from 30^(@)C to 60^(@)C at constant pressure. Heat given to the gas is (given R = 2 cal//mol degrees)

Temperature of one mole of a gas is increased by 1^(@) C at constant pressure. The work done on the system is

Q cal of heat is required to raise the temperature of 1 mole of a monatomic gas from 20^(@)C to 30^(@)C at constant pressure. The amount of heat required to raise the temperature of 1 mole of diatomic gas form 20^(@)C to 25^(@)C

Temperature of 1 mole of a gas is increased by 2^(@)C at constant pressure. Work done is :

For one mole of an ideal gas, increasing the temperature from 10^(@)C to 20^(@)C

The work done by one mole of ideal gas when its teperature is increased by 1^oC at constant pressure is

The ammount of heat required to raise the temperature of 1 mole of diatomic gas by 1^(@)C at constant pressure is 60cal . The amount of heat which goes as internal energy of the gas is nearly.

How much heat energy should be added to the gaseous mixture consisting of 1 g of hydrogen and 1g of helium to raise it s temperature from 0^(@)C to 100^(@)C (a) at constant volume, b. at constant pressure (R = 2 cal//mol K) ?

The change in internal energy when 5 mole of hydrogen is heated to 20^(@)C from 10^(@)C , specific heat of hydrogen at constant pressure is 8 cal/mol .^(@)C is