Calculate the entropy change involved in the conversion of one mole of water at `373 K` to vapour at the same temperature.(Latent heat of vaporisation of water at this temperature , `Delta H_vap = 2.257 kJg^-1`)

Calculate the entropy change when 1 gram of ice is converted to water. Given triangleH=6025 J/mole

The entropy change for vaporisation of liquid water to steam at 100^@C is _____ JK^-1 mol^-1 , Given that heat of vapori-sation is 40.8kJ mol^-1 .

One gm of water at 373 K is converted into steam at the same temperature. The volume of 1 c .c of water becomes' 1671 c.c on boiling. Calculate the change in internal energy of the system if heat of vaporisation of water is 5.4xx10^5calkg^-1 .

A vessel has nitrogen gas and water vapours at a total pressure of 1 atm. The partial pressure of water vapours is 0.3 atm. The contents of this vessel are transferred to another vessel havig one third of the capacity of original volume, completely at the same temperature, the total pressure of the system in the new vessel is :

500mL of a hydrocarbon gas burnt in excess of oxygen yielded 2500 mL of Co_2 and 3.0 liter of water vapour (all volumes measured at the same temperature and pressure). The formula of the hydrocarbon is :

One mole of a gas absorbs 200 J of heat at constant volume. Its temperature rises from 298 K to 308 K. The change in internal energy is:

A and B are two identical vessels. A contains 15 g of ethene at 298 K and 1 atm. The vessel B contains 75 g gas X_2 at the same temperature and pressure. The vapour density of X_2 is :

Latent heat of vaporisation of a liquid at 500K and 1 atm pressure is 10.0 kcal/mol. What will be the change in internal energy (triangleE) of 3 mole of liquid at same temperature: