3moles of a diatomic gas are heated from `127^(@)C` to `727^(@)C` at a constant pressure of 1 atm.Entropy change is (log2.5=0.4)

One mole of an ideal gas is heated from 0^@ C to 100^@ C at a constant pressure of 1 atmosphere. Calculate the work done in the process.

5 moles of an ideal monoatomic gas absorbes x joule when heated from 25^(@) C to 30^(@) C at a constant volume. The amount of heat absorbed when 2 moles of the same gas is heated from 25^(@) C to 30^(@) C at constant pressure, 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

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 from 20^(@)C to 25^(@)C at constant pressure is

Four moles of a diatomic gas is heated from 0^@C to 50^@C , find the heat supplies to the gas if work done by it is zero.

Four moles of a diatomic gas is heated from 0 ^@ C to 50^@ C . Find the heat supplied to the gas if work done by it is zero.

If 294 joules of heat energy is required to raise the temperature of 2 moles of an ideal gas from 30^(@)C to 35^(@)C at constant pressure, then the specific heat at constant pressure will be (R=8.4J/mol .^(@)K )

For one mole of a diatomic gas, the ratio of heat transfer at constant pressure to work done by the gas is

The temperature and pressure of one mole of an ideal monoatomic gas changes from 25^(@) C and 1 atm pressure to 250^(@) C and 25 atm. Calculate the change in entropy for the process.

One mole of water at 100^@ C is converted into steam at 100^@ C at a constant pressure of 1 atm. The change in entropy is ____________. (heat of vaporization of water at 100^@ C=540 cal/g)