Chapter 18, Problem 18.13QP

Interpretation Introduction

Interpretation: The following reagent should be identified which can oxidase ${\text{H}}_{\text{2}}\text{O}$ to ${\text{O}}_2$(g) under standard state condition.

Concept Introduction:

Electrolysis is the use of electric energy to drive a nonspontaneous redox reaction. An electrochemical cell used for this purpose is called an electrolytic cell.

Redox reaction are those in which oxidation number changes.

Half reaction are the separated oxidation and reduction reaction that make up the overall redox reaction.

Redox equation can be balanced via the half –reaction methods, which allows for the addition of ${\text{H}}_{\text{2}}\text{O}$ to balance O, ${\text{H}}^{+}$ to balance H, and ${\text{OH}}^{-}$ for taking place in basic solution.

Standard EMF:

The electromotive force (EMF) is the maximum potential difference between two electrodes of a galvanic cell.

This quantity is related to the tendency for an element.

i.e- It has a great tendency to acquire or gain the compound.

Half-cell Reaction: A half-cell is one of the two electrodes in a galvanic cell.

Example, the Zn-Cu battery, the two half cells make an oxidizing couple.

Electrochemical cell:

An electrochemical cell in which a spontaneous chemical reaction generates a flow of electrons through a wire is called a galvanic cell

To identify: The following reagent which is responsible to convert water molecule into oxygen molecule.