Question

given E^o= -0.13v and E^o cu2+,cu=0.34v construct cell and wrote cell cycle​

Answer 1

Explanation:

determine relative oxidizing and reducing strengths of a series of metals and ions.

GOALS

1

To explore the relative oxidizing and reducing strengths of different metals.

2

To gain practice working with electrochemical cells.

3

To use experimentally determined cell potentials to rank reduction half-reactions.

INTRODUCTION

The movement or transfer of electrons is central to our understanding of chemical reactions. The study of the transfer of electrons from one reactant to another is the study of electrochemistry. Electrons can move spontaneously from higher energy levels to lower energy levels within an atom. A similar movement can take place between two different chemical reactants. If there are electrons in one reactant that are at higher energy than unfilled orbitals of the other reactant, the high energy electrons can transfer to the unfilled orbitals at lower energy. This transfer of electrons from one chemical substance to another is known as an oxidation-reduction (redox) or electron transfer reaction.

Consider the redox reaction (1) and Figure 1 below:

( 1 )

Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)

Figure 1

Figure 1: Energy Diagram for Reaction between Zinc Metal and Copper(II) Ion.

One reactant, zinc metal, has a pair of electrons at a much higher energy level than an unfilled orbital in the other reactant, copper(II) ion. The electrons in the higher energy orbital in zinc can spontaneously move to the lower energy orbital in