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: Which of the electrode is negatively charged?

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

Given the standard electrode potentials,
\(K^{+}/K = –2.93V\), \(Ag^{+}/Ag = 0.80V\),
\(Hg^{2+}/Hg = 0.79V\)
\(Mg^{2+}/Mg = –2.37 V\), \(Cr^{3+}/Cr = – 0.74V\)
Arrange these metals in their increasing order of reducing power.

Conductivity of 0.00241 M acetic acid is \(7.896 \times 10^{-5} S cm^{-1}\). Calculate its molar conductivity. If \(\Lambda_{m}^{\circ}\) for acetic acid is \(390.5 S cm^{2} mol^{-1}\), what is its dissociation constant?

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.

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

Write the Nernst equation and emf of the following cell at 298 K:
\(Mg(s)|Mg^{2+}(0.001M)||Cu^{2+}(0.0001 M)|Cu(s)\)

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

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

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

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:
\(Fe^{2+}(aq) + Ag^{+}(aq) \rightarrow Fe^{3+}(aq) + Ag(s)\)
Calculate the \(\Delta_{r}G^{\circ}\) and equilibrium constant of the reaction.

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

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.

DNA fragments are

Using the standard electrode potentials given in Table 3.1, predict if the reaction between the following is feasible: \(Br_{2} (aq)\) and \(Fe^{2+} (aq)\).

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: An aqueous solution of \(AgNO_{3}\) with silver electrodes.

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