The conductivity of 0.20 M solution of KCl at 298 K is \(0.0248 S cm^{-1}\). Calculate its molar conductivity.

How much electricity in terms of Faraday is required to produce 20.0 g of Ca from molten \(CaCl_{2}\)?

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.

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 \(MnO_{4}^{-}\) to \(Mn^{2+}\)?

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

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

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

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

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?

Arrange the following metals in the order in which they displace each other from the solution of their salts.
Al, Cu, Fe, Mg and Zn.

How much electricity is required in coulomb for the oxidation of 1 mol of FeO to \(Fe_{2}O_{3}\)?

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

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

How much electricity is required in coulomb for the oxidation of 1 mol of \(H_{2}O\) to \(O_{2}\)?

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.

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.

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

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

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