$N{i}_2{O}_3\left(s\right)+H_{2}O\left(l\right)+2e^{-}\to 2NiO\left(s\right)+2O{H}^{-}\left(aq\right)$  $E^0=0.4V$

$FeO\left(s\right)+H_{2}O\left(l\right)+2e^{-}\to Fe\left(s\right)+2O{H}^{-}\left(aq\right)$  $E^0=-0.87V$

The overall reaction for the spontaneous cell has a value of  $\Delta H^0=-490kJ/mol$
Which of the following option(s) is/are correct?

Cell reaction is  $N{i}_2{O}_3\left(s\right)+Fe\left(s\right)\to 2NiO\left(s\right)+FeO\left(s\right)$

$E_{cell}^0$ is 1.27 V

Efficiency of cell is 50.02 %

The maximum amount of electrical energy that can be obtained is equal to 245.11 kJ per mole of formation of Nickel(II) oxide