   Chapter 19.2, Problem 19.4CYU

Chapter
Section
Textbook Problem

The following overall chemical reaction occurs in an electrochemical cell.Overall chemical equation: Zn(s) + PbSO4(s) → Zn2+(aq) + Pb(s) + SO42−(aq)Use cell notation to describe the electrochemical cell.

Interpretation Introduction

Interpretation:

The electrochemical cell has to be described using cell notation.

Zn(s) + PbSO4(s) Zn2+(aq) + pb(s) + SO42-(aq)

Concept introduction:

Electrochemical cells:

Cells in which chemical energy get converted into electrical energy.

In all electrochemical cells, oxidation occurs at anode and reduction occurs at cathode.

An anode is indicated by negative sign and cathode is indicated by the positive sign.

Electrons flow in the external circuit from the anode to the cathode.

In the electrochemical cells two half cells are connected with salt bridge. It allows the cations and anions to move between the two half cells.

Under certain conditions a cell potential is measured it is called as standard potential (Ecello).

Standard potential (Ecello) can be calculated by the following formula.

Ecello=Ecathodeo-Eanodeo

The Ecello value is positive; the reaction is predicted to be product favoured at equilibrium.

The Ecello value is negative; the reaction is predicted to be reactant favoured at equilibrium.

Explanation

The given reaction is as follows.

Zn(s) + PbSO4(s) Zn2+(aq) + pb(s) + SO42-(aq)

Let’s write the half reactions:

At anode:Oxidation:  Zn(s) Zn2+(s) +2e-

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