70 cals of heat is required to raise the temperature of 2 moles of an ideal gas at constant pressure from `30^@C` to `35^@C`. Calculate the amount of heat required to raise the temperature of same gas through same range at constant volume. (R = 2 cal / mole `^@C`)

70 cal of heat is required to raise the temperature of 20 moles of an ideal diatomic gas at constant pressure from 30^@C . The amount of heat required (in cal) to raise the temperature of the same gas through the same range ( 30^@C to 35^@C ) at constant volume is

70 cal of heat is required to increase the temperature of 2 mol of an ideal diatomic gas at constant pressure from 40^(@)C to 45^(@)C . How much heat will be required to increase the temperature of that gas by the same amount at constant volume? R = 2 cal cdot mol^(-1) cdot K^(-1) .

Amount of heat required to raise the temperature of 1 kg of water by 1^@C is

The amount of heat energy required to raise the temperature of 1g of water b 1^@C is called

One mole of an ideal monoatomic gas is heated at constant pressure from 0^@C to 100^@C . Calculate work done.

Why is the pressure of a given amount of gas increased when the temperature of the gas is raised at constant volume?

The work done by an ideal gas at constant temperature is 10 J. the amount of heat gained in this process is

How much heat is required to raise the temperature of 90 g of water from 30^(@)C to 100^(@)C ? [Molar heat capacity of water at constant pressure =75.3J*mol^(-1)*K^(-1) ]