What is the entropy change (in JK ^-1 mol ^-1), when one mole of ice is converted into water at 0^oC? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol ^-1 at 0^oC.)  

A gas present in a cylinder, fitted with a frictionless piston, expands against a constant pressure of 1 atm from a volume of 2 liter to a volume of 6 liter. In doing so, it absorbs 800 J heat from surroundings. The increase in internal energy of process is 

When one mole of monoatomic ideal gas at T K undergoes adiabatic change under a constant external pressure of 1 atm, changes volume from 1L to 2L. The final temperature in Kelvin would be   

Mercury thermometer can be used to measure temperature up to  

When 1.8 g of steam at the normal boiling point of water is converted into water, at the same temperature, enthalpy and entropy changes respectively will be

[ Given ∆H_vap for water = 40.8kJ mol^-1 ]

 When I mole of a gas is heated at constant volume, temperature is raised from 298 K to 308 k. Heat supplied to the gas is 500 J. Then, which statement is correct? 

At 27^oC latent heat of fusion of a compound is 2930 J/mol. Entropy change during fusion is  

In which process net work done is zero? 

The value of log₁₀ K for a reaction A   B is

         (Given, ∆_rH^o_{298 K} = - 54.07 kJ mol ^-1

                        ∆_rS^o_{298 k} = 10 JK ^-1 mol ^-1

         and                        R = 8.314 JK ^-1 mol ^-1

                                          = 2.303 x 8.314 x 298

                                           = 5705