Chapter 21.3, Problem 21.3BFP

Interpretation Introduction

Interpretation:

The given ionic reaction has to be balanced and the $E^{\circ }{}_{cell}$ has to be calculated to decide whether the given reaction is spontaneous or not.

Concept Introduction:

An electrochemical cell is a device in which a redox reaction is used to convert chemical energy into electrical energy. Such device is also known as the galvanic or voltaic cell.

Galvanic cell consists of two half-cells. The redox reaction occurs in these half-cells. The half-cell in which the reduction reaction occurs is known as the reduction half-cell, whereas the half-cell in which the oxidation reaction occurs is known as the oxidation half-cell.

The standard cell potential for voltaic cell is determined by subtracting the electrode potential of cathode and the electrode potential of cathode.

The negative cell potential of a redox reaction indicates that the reaction is not spontaneous which shows that the standard free energy should be less than 0. The reverse reaction of this will be definitely a spontaneous reaction with cell potential value greater than 0.

• Chemical equation is the representation of a chemical reaction, in which the reactants and products of the reactions are represented left and right side of an arrow respectively by using their respective chemical formulas.
• Reactant of a chemical reaction is the substrate compounds or the compounds which undergo a chemical reaction.
• Product of a chemical reaction is the produced compounds or the compounds formed after a chemical reaction.
• Balanced chemical equation of a reaction is written according to law of conservation of mass.
• Stoichiometry of a chemical reaction is the relation between reactants and products of the reaction and it is represented by the coefficients used for the reactants and products involved in the chemical equation.