\(\Delta H^\circ = -296 \, \text{kJ} - (3 \times 8.3 \, \text{J K}^{-1} \text{mol}^{-1} \times 298 \, \text{K} \times 10^{-3}) \approx -303.42 \, \text{kJ}\)
\(\Delta H^\circ(\text{HgO(s)}) = \Delta H^\circ(\text{HgO(s)}) - \Delta H^\circ(\text{Hg(g)}) - 2 \times \Delta H^\circ(\text{Hg(s)})\)
\(\Delta H^\circ(\text{HgO(s)}) = -303.42 + 122.64 - 180.78 = -303.42 + 90.39 \, \text{kJ mol}^{-1}\)
Thus, the absolute value of the enthalpy of formation for solid mercury oxide HgO(s)) is 90.39 kJ mol−1.
A perfect gas (0.1 mol) having \( \bar{C}_V = 1.50 \) R (independent of temperature) undergoes the above transformation from point 1 to point 4. If each step is reversible, the total work done (w) while going from point 1 to point 4 is ____ J (nearest integer) [Given : R = 0.082 L atm K\(^{-1}\)]
A sample of n-octane (1.14 g) was completely burnt in excess of oxygen in a bomb calorimeter, whose heat capacity is 5 kJ K\(^{-1}\). As a result of combustion, the temperature of the calorimeter increased by 5 K. The magnitude of the heat of combustion at constant volume is ___
An electrochemical cell is a device that is used to create electrical energy through the chemical reactions which are involved in it. The electrical energy supplied to electrochemical cells is used to smooth the chemical reactions. In the electrochemical cell, the involved devices have the ability to convert the chemical energy to electrical energy or vice-versa.