$Zn_{(s)} + Ag_2O_{(s)} + H_2O_{(l)} \rightleftharpoons $$2Ag_{(s)} + Zn^{2+}_{(aq)}+ 2OH^-_{(aq)}$
If half cell potentials are
$Zn^{2+}_{(aq)} + 2e^- \rightarrow Zn_{(s)}\,;\,\, E^o = - 0.76\, V$
$Ag_2O_{(s)} + H_2O_{(l)} + 2e^- \rightarrow 2Ag_{(s)} + 2OH^-_{(aq)}\,,$$E^o = 0.34\, V$
The cell potential will be ........... $V.$
$=0.76+0.34=1.10 \mathrm{V} $
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${N_2}{H_4}\left( l \right) + 2{H_2}{O_2}\left( l \right) \to \mathop {{N_2}\left( g \right) + 4{H_2}O\left( l \right);}\limits_{{\Delta_r} H_1^o = - 818\,kJ/mol} $
${N_2}{H_4}\left( l \right) + {O_2}\left( g \right) \to \mathop {{N_2}\left( g \right) + 2{H_2}O\left( l \right);}\limits_{{\Delta _r}H_2^o = - 622\,kJ/mol} $
${H_2}\left( g \right) + \frac{1}{2}{O_2}\left( g \right) \to \mathop {{H_2}O\left( l \right);}\limits_{{\Delta _r}H_3^o = - 285\,kJ/mol} $
.......$kJ/mol$