Electrochemistry

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 gas liberated by the electrolysis of Dipotassium succinate solution is :

How many electrons would be required to deposit 6.35 g of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate ? (Atomic mass of copper = 63.5 u, $N_A$ = Avogadro's constant) :

The standard reduction potential data at 25 °C is given below.

$E^\circ(\ce{Fe^{3+}},\ce{Fe^{2+}})=+0.77$ V; $E^\circ(\ce{Fe^{2+}},\ce{Fe})=-0.44$ V;
$E^\circ(\ce{Cu^{2+}},\ce{Cu})=+0.34$ V; $E^\circ(\ce{Cu+},\ce{Cu})=+0.52$ V;
$E^\circ[\ce{O2(g) + 4H+ + 4e- -> 2H2O}]=+1.23$ V; $E^\circ[\ce{O2(g) + 2H2O + 4e- -> 4OH-}]=+0.40$ V;
$E^\circ(\ce{Cr^{3+}},\ce{Cr})=-0.74$ V; $E^\circ(\ce{Cr^{2+}},\ce{Cr})=-0.91$ V

Match $E^\circ$ of the redox pair in List I with the values given in List II and select the correct answer using the code given below the lists:

An aqueous solution of X is added slowly to an aqueous solution of Y as shown in List I. The variation in conductivity of these reactions is given in List II. Match List I with List II and select the correct answer using the code given below the lists:

The solubility product ($K_{sp}$; mol³ dm⁻⁹) of $\ce{MX2}$ at 298 K based on the information available for the given concentration cell is (take $2.303\times R\times298/F=0.059$ V)

The value of $\Delta G$ (kJ mol⁻¹) for the given cell is (take 1 F = 96500 C mol⁻¹)

$\ce{AgNO3}$(aq.) was added to an aqueous KCl solution gradually and the conductivity of the solution was measured. The plot of conductance ($\Lambda$) versus the volume of $\ce{AgNO3}$ is

The metal rod M is

Consider the following cell reaction:
$$\ce{2Fe(s) + O2(g) + 4H+(aq) -> 2Fe^{2+}(aq) + 2H2O(l)}\qquad E^\circ=1.67\ \mathrm V$$
At $[\ce{Fe^{2+}}]=10^{-3}$ M, $P(\ce{O2})=0.1$ atm and pH = 3, the cell potential at 25 °C is

Among the following, the intensive property is (properties are)

For the above cell

If the 0.05 molar solution of $\ce{M+}$ is replaced by a 0.0025 molar $\ce{M+}$ solution, then the magnitude of the cell potential would be

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)

Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 milli ampere current. The time required to liberate 0.01 mol of $\ce{H2}$ gas at the cathode is (1 Faraday = 96500 C mol⁻¹)

The total number of moles of chlorine gas evolved is

If the cathode is a Hg electrode, the maximum weight (g) of amalgam formed from this solution is

The total charge (coulombs) required for complete electrolysis is

Among the following, identify the correct statement.

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