At 1 atm pressure, ∆S = 75 JK ^-1 mol ^-1;  ∆H = 30 kJ mol ^-1. The temperature of the reaction at equilibrium is 

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

For a reaction 

∆H = 30 kJ mol ^-1 and  ∆S = 0.07 kJ K ^-1 mol ^-1 at 1 atm. The temperature up to which the reaction would not be spontaneous is   

When the heat of a reaction at constant pressure is -2.5 x 10³ cals and entropy change for the reaction is

7.4 cal deg ^-1, it is predicted that the reaction at 25^oC is

Spontaneous adsorption of a gas on solid surface is an exothermic process because 

For a particular reversible reaction at temperature T, ∆H and ∆S were found to be both +ve. If T_e is the temperature at equilibrium, the reaction would be spontaneous when  

110J of heat is added to a gaseous system, whose internal energy is 40J, then the amount of external work done is 

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 

Standard enthalpy and standard entropy change for the oxidation of NH₃ at 298 K, are -382.64 mol ^-1 and -145.6 J mol ^-1 respectively. Standard Gibbs energy change for the same reaction at 298 K is