A monoatomic ideal gas undergoes a process in which the ratio of p to V at any instant is constant and equals to 1. What is the molar heat capacity of the gas?   

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   

The molar heat capacity of water at constant pressure is 75 JK ^-1 mol ^-1. When 1.0 kJ of heat is supplied to 100 g of water, which is free to expand, the increase in temperature of water is    

Mercury thermometer can be used to measure temperature up to  

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

Statement I  All exothermic reactions are spontaneous at room temperature.

Statement II In (∆G = ∆H - T∆S), ∆G becomes negative and negative sign of ∆G indicates spontaneous reaction.

In conversion of limestone to lime,

              C_aCO₃ (s) → C_aO(s) + CO₂ (g)

The value of ∆H^o and ∆S^o are  +179.1 kJ mol ^-1 and  160.2 J/ K respectively at 298 K and 1 bar. Assuming that ∆H^o and ∆S^o do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is

Standard entropy of X₂, Y₂ and XY₃ are 60, 40 and 50 JK ^-1 mol ^-1 respectively. For the reaction     to be at the equilibrium, the temperature will be

2 moles of an ideal gas at 27^oC are expanded reversibly from 2 L to 20 L. Find entropy change. (R = 2 cal/ mol K)

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