If $E^{\circ}_{Fe^{2+}/Fe} = -0.440 \ V$ and $E^{\circ}_{Fe^{3+}/Fe^{2+}} = 0.770 \ V$,then $E^{\circ}_{Fe^{3+}/Fe}$ is (in $V$)

Review the $SRP$ (at $25\,\text{°C}$) data in acidic medium:
$Ti^{4+} + e^- \to Ti^{3+}, \, E^o = -x \text{ V}$
$Fe^{3+} + e^- \to Fe^{2+}, \, E^o = -y \text{ V}$
where $x < y$,point out the wrong statement.

Fill in the blanks :
$1$. ...... metal is the strongest reducing agent in aqueous solution.
$2$. ...... gas is the strongest oxidizing agent.
$3$. The standard reduction potential of any electrode is measured with reference to ......

Calculate the $emf$ of the cell $Cu_{(s)} | Cu^{2+}_{(aq)} || Ag^+_{(aq)} | Ag_{(s)}$. Given: $E^0_{Cu^{2+}/Cu} = +0.34 \ V$,$E^0_{Ag^+/Ag} = +0.80 \ V$.

For a Galvanic cell consisting of a zinc electrode and a standard hydrogen electrode,$E^{\circ}(Zn^{+2}_{(aq)} \mid Zn_{(s)}) = -0.76 \ V$. Identify the reaction that takes place at the positive electrode during the working of the cell.

Assertion : Copper reacts with $HCl$ and liberates hydrogen.
Reason : Hydrogen is present above $Cu$ in the reactivity series.