How many calories are required to increase the temperature of 40g of Ar from `40^(@)C` to `100^(@)C` at a constant volume `(R=2cal*mol^(-1)*K^(-1))`-

How many calories are required to heat 40 g of argon from 40^(@)C to 100^(@)C at constant volume? (R = 2 cal mol^(-1) K^(-1))

1 calorie is the heat required to increased the temperature of 1 gm of water by 1°C from

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) .

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) ]

Amount of heat energy required to raise the temperature of 2 g neon gas by 54°F at constant volume is (R= 2 cal mol^-1 K^-1 )

Amount of heat energy required to raise the temperature of 2 g neon gas by 54°F at constant volume is (R= 2 cal mol^-1 K^-1 )

H calories of heat is required to increase the temperature of one mole of monoatomis gas from 20^(@)C" to "30^(@)C at const. volume. The quantity of heat required to increase the temperature of 2 moles of a diatomic gas from 20^(@)C" to "25^(@)C is at constant volume is

Calculate the amount of heat energy required to increase the temperature of 250 g of water from 27^(@)C to 67^(@)C (Specific heat capacity of water is 1 cal g^(-1@)C^(-1) )