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

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))

Calculate DeltaU and DeltaH in calories if one mole of a monoatomic ideal gas is heated at constant pressure of 1 atm from 25^(@)C to 50^(@)C .

The temperature of 1 mol of an ideal monoatomic gas at constant pressure of 1 atm changes from 25^(@)C and 50^(@)C . Calculate Delta U and Delta H in this process, (C_(V)=(3)/(2)R) .

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 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) .

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