Statement 1 : There is a natural asymmetry between converting work to heat and converting heat to work.

Statement 2 : No process is possible in which the sole result is the absorption of heat from a reservoir and its complete conversion into work.

For the process $$\mathrm{H_2O}(l)$$ (1 bar, 373 K) $$\to$$ $$\mathrm{H_2O}(g)$$ (1 bar, 373 K), the correct set of thermodynamic parameters is:

The value of log$$_{10}$$ K for a reaction $A \rightleftharpoons B$ is

(Given : $${\Delta _r}H{^\circ _{298\,K}} = - 54.07$$ kJ mol$$^{-1}$$, $${\Delta _r}S{^\circ _{298\,K}} = 10$$ J K$$^{-1}$$ mol$$^{-1}$$ and R = 8.314 J K$$^{-1}$$ mol$$^{-1}$$; 2.303 $$\times$$ 8.314 $$\times$$ 298 = 5705)

A monatomic 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?