\(\Delta H^\circ = -296 \, \text{kJ} - (3 \times 8.3 \, \text{J K}^{-1} \text{mol}^{-1} \times 298 \, \text{K} \times 10^{-3}) \approx -303.42 \, \text{kJ}\)
\(\Delta H^\circ(\text{HgO(s)}) = \Delta H^\circ(\text{HgO(s)}) - \Delta H^\circ(\text{Hg(g)}) - 2 \times \Delta H^\circ(\text{Hg(s)})\)
\(\Delta H^\circ(\text{HgO(s)}) = -303.42 + 122.64 - 180.78 = -303.42 + 90.39 \, \text{kJ mol}^{-1}\)
Thus, the absolute value of the enthalpy of formation for solid mercury oxide HgO(s)) is 90.39 kJ mol−1.
The solubility of barium iodate in an aqueous solution prepared by mixing 200 mL of 0.010 M barium nitrate with 100 mL of 0.10 M sodium iodate is $X \times 10^{-6} \, \text{mol dm}^{-3}$. The value of $X$ is ------.
Use: Solubility product constant $(K_{sp})$ of barium iodate = $1.58 \times 10^{-9}$
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.