Galvanic cells and EMF

What will occur if a block of copper metal is dropped into a beaker containing a solution of 1M $\ce{ZnSO4}$ ?

Identify the correct statement :

A variable, opposite external potential ($E_{ext}$) is applied to the cell $\ce{Zn | Zn^2+ (1 M) || Cu^2+ (1 M) | Cu}$, of potential 1.1 V. When $E_{ext}<1.1$ V and $E_{ext}>1.1$ V, respectively electrons flow from :

In a galvanic cell, the salt bridge

Given below are the half - cell reactions :

$\ce{Mn^2+ + 2e- -> Mn}$ ; $E^\circ=-1.18$ V

$2\left(\ce{Mn^3+ + e- -> Mn^2+}\right)$ ; $E^\circ=+1.51$ V

The $E^\circ$ for $\ce{3Mn^2+ -> Mn + 2Mn^3+}$ will be :

The standard electrode potentials $\left(E^\circ_{\ce{M+}/\ce{M}}\right)$ of four metals A, B, C and D are $-1.2$ V, 0.6 V, 0.85 V and $-0.76$ V, respectively. The sequence of deposition of metals on applying potential is :

Given

$\ce{Fe^3+(aq) + e- -> Fe^2+(aq)}$; $E^\circ=+0.77$ V

$\ce{Al^3+(aq) + 3e- -> Al(s)}$; $E^\circ=-1.66$ V

$\ce{Br2(aq) + 2e- -> 2Br-}$; $E^\circ=+1.09$ V

Considering the electrode potentials, which of the following represents the correct order of reducing power ?

The metal rod M is

For the reduction of $\ce{NO3-}$ ion in an aqueous solution, $E^\circ$ is +0.96 V. Values of $E^\circ$ for some metal ions are given below

Half-reaction	$E^\circ$
$\ce{V^{2+}(aq) + 2e- -> V}$	−1.19 V
$\ce{Fe^{3+}(aq) + 3e- -> Fe}$	−0.04 V
$\ce{Au^{3+}(aq) + 3e- -> Au}$	+1.40 V
$\ce{Hg^{2+}(aq) + 2e- -> Hg}$	+0.86 V

The pair(s) of metals that is(are) oxidized by $\ce{NO3-}$ in aqueous solution is(are)

Among the following, identify the correct statement.

While $\ce{Fe^{3+}}$ is stable, $\ce{Mn^{3+}}$ is not stable in acid solution because