The conductivity of sodium chloride at 298 K has been determined at different concentrations and the results are given below: 

Calculate \(\Lambda_{m}\) for all concentrations and draw a plot between \(\Lambda_{m}\) and \(c^{1/2}\). Find the value of \(\Lambda_{m}^{\circ}\).

Depict the galvanic cell in which the reaction \(Zn(s)+2Ag^{+}(aq) \rightarrow Zn^{2+}(aq)+2Ag(s)\) takes place. Further show: The carriers of the current in the cell.

Three electrolytic cells A,B,C containing solutions of \(ZnSO_{4}\), \(AgNO_{3}\) and \(CuSO_{4}\), respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?

In a galvanic cell, the positive terminal electrode is known as 

Write the Nernst equation and emf of the following cell at 298 K:
\(Fe(s)|Fe^{2+}(0.001M)||H^{+}(1M)|H_{2}(g)(1bar)| Pt(s)\)

Predict the products of electrolysis in each of the following: An aqueous solution of \(AgNO_{3}\) with platinum electrodes.

Write the Nernst equation and emf of the following cell at 298 K:
\(Sn(s)|Sn^{2+}(0.050 M)||H^{+}(0.020 M)|H_{2}(g) (1 bar)|Pt(s)\)

Write the Nernst equation and emf of the following cell at 298 K:
\(Pt(s)|Br^{-}(0.010 M)|Br_{2}(l )||H^{+}(0.030 M)| H_{2}(g) (1 bar)|Pt(s)\).

Define conductivity and molar conductivity for the solution of an electrolyte. Discuss their variation with concentration.

A solution of \(Ni(NO_{3})_{2}\) is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?

In the button cells widely used in watches and other devices the following reaction takes place:
\(Zn(s) + Ag_{2}O(s) + H_{2}O(l ) \rightarrow Zn^{2+}(aq) + 2Ag(s) + 2OH^{-}(aq)\)
Determine \(\Delta_{r}G^{\circ}\) and \(E^{\circ}\) for the reaction.

How much charge is required for the following reduction:
1 mol of \(MnO_{4}^{-}\) to \(Mn^{2+}\)?

Using the standard electrode potentials given in Table 3.1, predict if the reaction between the following is feasible: \(Fe^{3+} (aq)\) and \(Br^{-} (aq)\)

Depict the galvanic cell in which the reaction \(Zn(s)+2Ag^{+}(aq) \rightarrow Zn^{2+}(aq)+2Ag(s)\) takes place. Further show: Individual reaction at each electrode.

How much charge is required for the following reduction:
1 mol of \(Cu^{2+}\) to Cu?

DNA fragments are

How much charge is required for the following reduction:
1 mol of \(Al^{3+}\) to Al?

Predict the products of electrolysis in each of the following: An aqueous solution of \(CuCl_{2}\) with platinum electrodes.

Calculate the standard cell potentials of galvanic cell in which the following reaction takes place:
\(2Cr(s) + 3Cd^{2+}(aq) \rightarrow 2Cr^{3+}(aq) + 3Cd(s)\)
Calculate the \(\Delta_{r}G^{\circ}\) and equilibrium constant of the reaction.

Predict the products of electrolysis in each of the following: A dilute solution of \(H_{2}SO_{4}\) with platinum electrodes.