An aqueous solution of hydrazine $\left(\mathrm{N}_2 \mathrm{H}_4\right)$ is electrochemically oxidized by $\mathrm{O}_2$, thereby releasing chemical energy in the form of electrical energy. One of the products generated from the electrochemical reaction is $\mathrm{N}_2(\mathrm{~g})$.

Choose the correct statement(s) about the above process

In a conductometric titration, small volume of titrant of higher concentration is added stepwise to a larger volume of titrate of much lower concentration, and the conductance is measured after each addition.

The limiting ionic conductivity $\left(\Lambda_0\right)$ values (in $\mathrm{mS} \mathrm{m}{ }^2 \mathrm{~mol}^{-1}$ ) for different ions in aqueous solutions are given below:

$ \begin{array}{|c|c|c|c|c|c|c|c|c|c|} \hline \text { Ions } & \mathrm{Ag}^{+} & \mathrm{K}^{+} & \mathrm{Na}^{+} & \mathrm{H}^{+} & \mathrm{NO}_3^{-} & \mathrm{Cl}^{-} & \mathrm{SO}_4^{2-} & \mathrm{OH}^{-} & \mathrm{CH}_3 \mathrm{COO}^{-} \\ \hline \Lambda_0 & 6.2 & 7.4 & 5.0 & 35.0 & 7.2 & 7.6 & 16.0 & 19.9 & 4.1 \\ \hline \end{array} $

For different combinations of titrates and titrants given in List-I, the graphs of 'conductance' versus 'volume of titrant' are given in List-II.

Match each entry in List-I with the appropriate entry in List-II and choose the correct option.

LIST-I	LIST-II
(P) Titrate: KCl Titrant: AgNO$_3$
(Q) Titrate: AgNO$_3$ Titrant: KCl
(R) Titrate: NaOH Titrant: HCl
(S) Titrate: NaOH Titrant: CH$_3$COOH

The value of x is

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 AgNO₃ is

For the reduction of NO$_3^ - $ ion in an aqueous solution, E$^0$ is + 0.96 V. Values of E$^0$ for some metal ions are given below:

$\matrix{ {{V^{2 + }}(aq.) + 2{e^ - } \to V} & {{E^0} = - 1.19\,V} \cr {F{e^{3 + }}(aq.) + 3{e^ - } \to Fe} & {{E^0} = - 0.04\,V} \cr {A{u^{3 + }}(aq) + 3{e^ - } \to Au} & {{E^0} = + 1.40\,V} \cr {H{g^{2 + }}(aq) + 2{e^ - } \to Hg} & {{E^0} = + 0.86\,V} \cr } $

The pair(s) of metals that is (are) oxidized by NO$_3^ - $ 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 H$_2$ gas at the cathode is (1 Faraday = 96500 C mol$^{-1}$].

Among the following, identify the correct statement.

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

Sodium fusion extract, obtained from aniline, on treatment with iron (II) sulphate and $\mathrm{H}_{2} \mathrm{SO}_{4}$ in presence of air gives a Prussian blue precipitate. The blue colour is due to the formation of

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:

$ \begin{array}{r} 2 \mathrm{Ag}^{+}+\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6+\mathrm{H}_2 \mathrm{O} \rightarrow 2 \mathrm{Ag}(\mathrm{~s})+\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_7 +2 \mathrm{H}^{+} \end{array} $

Find $\ln \mathrm{K}$ of this reaction.

When ammonia is added to the solution, pH is raised to 11 . Which half-cell reaction is affected by pH and by how much?

Ammonia is always added in this reaction. Which of the following must be incorrect?