If `50 cal` of heat is supplied to the system containing `2 mol` of an ideal monatomic gas, the rise in temperature is `(R = 2 cal//mol-K)`

If 50 cal of heat is supplied at constant pressure to the system containing 2 mol of an ideal monatomic gas, the rise in temperature is (R = 2 cal//mol-K)

1672 cal of heat is given to one mole of oxygen at 0^(@)C keeping the volume constant. Rise in temperature is (R = 2 cal/mole/ ""^(@) K)

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 calories of heat is required to raise the temperature of 2 moles of an ideal gas at constant pressure from 40^(@)C to 45^(@)C (R=2cal/mol -.^(@)C ). The gas may be

70 calories of heat is required to raise the temperature of 2 moles of an ideal gas at constant pressure from 40^(@)C to 45^(@)C (R=2cal/mol -.^(@)C ). The gas may be

If 70 cal of heat is required to raise the temperature of moles of an ideal gas at constant pressure from 30^(@)C to 35^(@)C , calculate (i) the work done by the gas (ii) the increases in internal energy of the gas and (iii) degrees of freedom of gas molecules. given R =2 cal mol ^(-1) K^(-1)

50 cal of heat is required to raise the temperature of 1 mole of an ideal gas from 20^@ C to 25^@ C , while the pressure of the gas is kept constant. The amount of heat required to raise the temperature of the same has through same temperature range at constant volume is ( R = 2 cal/mol/K)