What is the standard electrode potential of a Daniell cell (in $V$)?

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.

Which chemical equation represents the standard reduction potential of zinc?

The $EMF$ of a cell in terms of the reduction potential of its left and right electrodes is:

The standard electrode potentials of $Ag^{+}/Ag$,$Hg_2^{2+}/2Hg$,$Cu^{2+}/Cu$,and $Mg^{2+}/Mg$ are $0.80 \ V$,$0.79 \ V$,$0.34 \ V$,and $-2.37 \ V$,respectively. An aqueous solution containing $1 \ M$ concentration of each of these metal salts is electrolyzed. With increasing voltage,what is the correct sequence of deposition of the metals at the cathode?

The standard electrode potential for the half-cell reactions are
$Zn^{2+} + 2e^{-} \longrightarrow Zn ; E^{\circ} = -0.76 \ V$
$Fe^{2+} + 2e^{-} \longrightarrow Fe ; E^{\circ} = -0.44 \ V$
The $emf$ of the cell reaction,
$Fe^{2+} + Zn \longrightarrow Zn^{2+} + Fe$ is