In the given button cell reaction, Zinc ($\text{Zn}$) is oxidised to $\text{Zn}^{2+}$ and silver oxide ($\text{Ag}_2\text{O}$) is reduced to silver ($\text{Ag}$). Therefore, the zinc electrode acts as the anode and the silver electrode acts as the cathode. The standard cell potential ($E^\circ_{\text{cell}}$) is calculated using the formula: $E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}}$ Given the standard reduction potentials: $E^\circ_{\text{cathode}} = 0.34 \text{ V}$ $E^\circ_{\text{anode}} = -0.76 \text{ V}$ Substituting these values into the formula: $E^\circ_{\text{cell}} = 0.34 \text{ V} - (-0.76 \text{ V}) = 0.34 + 0.76 = 1.10 \text{ V}$ The standard cell potential is $1.10 \text{ V}$.