A half-cell reaction represented by (i) below, namely 

$$\text{Fe(OH)}_2(s) + 2e^- \rightarrow \text{Fe}(s) + 2\text{OH}^-(aq)$$ with $$E^\circ = -0.9$$ V, takes place in two different electrochemical cells, I and II, in which the other half cell reactions are 

(ii) $$\text{Al}^{3+}(aq) + 3e^- \rightarrow \text{Al}(s)$$ with $$E^\circ = -1.7$$ V and 

(iii) $$\text{AgBr}(s) + e^- \rightarrow \text{Ag}(s) + \text{Br}^-(aq)$$ with $$E^\circ = -0.07$$ V respectively. 

The correct option that represents the redox reactions in cells I and II is