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

Given the standard electrode potentials, K⁺/K = -2.93V, Ag⁺/Ag = 0.80V, Hg²⁺/Hg = 0.79V Mg²⁺/Mg = -2.37 V, Cr³⁺/Cr = - 0.74VArrange these metals in their increasing order of reducing power.

Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺(aq) ? Zn²⁺(aq) + 2Ag(s) takes place. Further show: (I) Which of the electrode is negativelycharged? (II) The carriers of the current in thecell. (III) Individual reaction at each electrode.

Calculate the standard cell potentials of galvanic cells in which the following reactions take place: (i) 2Cr(s) + 3Cd²⁺(aq) ? 2Cr³⁺(aq) + 3Cd (ii) Fe²⁺(aq) + Ag⁺(aq) ? Fe³⁺(aq) + Ag(s) Calculate the ?_rG^? and equilibrium constant of the reactions.

Write the Nernst equation and emf of the following cells at 298 K: (i) Mg(s) | Mg²⁺(0.001M) || Cu²⁺(0.0001 M) | Cu(s) (ii) Fe(s) | Fe²⁺(0.001M) || H⁺(1M)|H₂(g)(1bar) | Pt(s) (iii) Sn(s) | Sn²⁺(0.050 M) || H⁺(0.020 M) | H₂(g) (1 bar) | Pt(s) (iv) Pt(s) | Br₂(l) | Br^-(0.010 M) || H⁺(0.030 M) | H₂(g) (1 bar) | Pt(s).

In the button cells widely used in watches and other devices the following reaction takes place: Zn(s) + Ag₂O(s) + H₂O(l) ? Zn²⁺(aq) + 2Ag(s) + 2OH^-(aq)Determine and for the reaction.

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

The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 Scm^-1. Calculate its molar conductivity.

The resistance of a conductivity cell containing 0.001M KCl solution at 298 K is 1500 ?. What is the cell constant if conductivity of 0.001M KCl solution at 298 K is 0.146 × 10^-3 Scm^-1.

The conductivity of sodium chloride at 298 K has been determined at different concentrations and the results are given below: Concentration/M 0.001 0.010 0.020 0.050 0.100 10² × ?/S m^-1 1.237 11.85 23.15 55.53 106.74 Calculatefor all concentrations and draw aplotbetweenand c½. Find the value of.

Conductivityof0.00241Maceticacidis7.896×10^-5Scm^-1.Calculateitsmolar conductivityandiffor acetic acid is 390.5 S cm² mol^-1, what is its dissociation constant?

How much charge is required for the following reductions: (I) 1 mol of Al³⁺ toAl. (II) 1 mol of Cu²⁺ toCu. (III) 1moloftoMn²⁺.

How much electricity in terms of Faraday is required to produce (I) 20.0 g of Ca from moltenCaCl₂. (II) 40.0 g of Al from moltenAl₂O₃.

How much electricity is required in coulomb for the oxidation of (I) 1 mol of H₂O toO₂. (II) 1 mol of FeO toFe₂O₃.

A solution of Ni(NO₃)₂ is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?

Three electrolytic cells A,B,C containing solutions of ZnSO₄, AgNO₃ and CuSO₄, 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 weredeposited?

Using the standard electrode potentials given in Table 3.1, predict if the reaction between the following isfeasible: (I) Fe³⁺(aq) andI^-(aq) (II) Ag⁺ (aq) and Cu(s) (III) Fe³⁺ (aq) and Br^-(aq) (IV) Ag(s) and Fe³⁺ (aq) (V) (aq) (aq)Br2 (aq) and Fe2+ (aq).

Predict the products of electrolysis in each of the following: (I) An aqueous solution of AgNO₃ with silverelectrodes. (II) An aqueous solution of AgNO₃with platinumelectrodes. (III) A dilute solution of H₂SO₄with platinumelectrodes. (IV) An aqueous solution of CuCl₂ with platinumelectrodes.

How would you determine the standard electrode potential of the systemMg2+ | Mg?

Can you store copper sulphate solutions in a zinc pot?

Consult the table of standard electrode potentials and suggest three substances that can oxidise ferrous ions under suitable conditions.

Calculate the potential of hydrogen electrode in contact with a solution whose pH is 10.

Calculate the emf of the cell in which the following reaction takes place: Given that = 1.05 V

The cell in which the following reactions occurs: has= 0.236 V at 298K. Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

Why does the conductivity of a solution decrease with dilution?

Suggest a way to determine the value of water.

The molar conductivity of 0.025 mol L-1 methanoic acid is 46.1 S cm2 mol^-1. Calculate its degree of dissociation and dissociation constant. Given ? ^°(H⁺)= 349.6 S cm2 mol-1 and ? °(HCOO-) = 54.6 S cm2 mol

If a current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons would flow through the wire?

Suggest a list of metals that are extracted electrolytically.

What is the quantity of electricity in coulombs needed to reduce 1 mol of ? Consider the reaction:

Suggest two materials other than hydrogen that can be used as fuels in fuel cells.

Explain how rusting of iron is envisaged as setting up of an electrochemical cell.