Four different solutions are placed in separate beakers,and a copper metal strip is added to each. Which solution will turn blue after some time?

Whose oxidation and reduction is carried out in a hydrogen-oxygen fuel cell?

Using the standard electrode potentials given in Table $3.1$ of the $NCERT$ textbook,predict if the reaction between the following is feasible:
$(i)$ $Fe^{3+}_{(aq)}$ and $I^{-}_{(aq)}$
$(ii)$ $Ag^{+}_{(aq)}$ and $Cu_{(s)}$
$(iii)$ $Fe^{3+}_{(aq)}$ and $Br^{-}_{(aq)}$
$(iv)$ $Ag_{(s)}$ and $Fe^{3+}_{(aq)}$
$(v)$ $Br_{2(aq)}$ and $Fe^{2+}_{(aq)}$

The reaction $1/2 H_{2(g)} + AgCl_{(s)} \to H^{+}_{(aq)} + Cl^{-}_{(aq)} + Ag_{(s)}$ occurs in the galvanic cell:

When a copper wire is placed in a solution of $AgNO_3$,the solution acquires a blue colour. This is due to the formation of

For a hydrogen-oxygen fuel cell at $1 \text{ atm}$ and $298 \text{ K}$, the reaction is $H_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow H_{2}O_{(l)}$; $\Delta G^{\circ} = -240 \text{ kJ}$. The $E^{\circ}$ for the cell is approximately (Given $F = 96,500 \text{ C}$): (in $\text{ V}$)