What were the concentrations of the solutions zinc solution

Question

Electrochemical Cells and Cell Potentials

Lab Report Assistant

This document is not meant to be a substitute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment's questions, diagrams if needed, and data tables that should be addressed in a formal lab report. The intent is to facilitate students' writing of lab reports by providing this information in an editable file which can be sent to an instructor.

Exercise 1: Construction of a Galvanic Cell

Data Table 1. Spontaneous Reaction Observations.

Metal in Solution	Observations
Zinc in Copper Sulfate	In the copper sulfate, the zinc turned black in color, my guess is corrosion occurred; this is a spontaneous reaction.
Copper in Zinc Sulfate	In the zinc sulfate, the copper did not show any noticeable changes; no spontaneous reaction occurred.

Data Table 2.Multimeter Readings.

Time (minutes)	Multimeter Reading (Volts)
0	1.07
15	1.07
30	1.07
45	1.08
60	1.08
75	1.08
90	1.08
105	1.08
120	1.07
135	1.07

Data Table 3. Standard Cell Potential.

	Equation	E°(Volts)
Oxidation Half-Reaction
Reduction Half-Reaction
Redox Reaction

Data Table 4. Galvanic Cell Setup.

Photograph of galvanic cell

Questions

A. What were the concentrations of the solutions (zinc solution, copper solution, and salt bridge)? Were the concentrations consistent with those of standard state conditions? Explain your answer.

B. Was the amount of electric energy produced in your galvanic cell consistent with the standard cell potential of the reaction (as calculated in Data Table 3)? Hypothesize why it was or was not consistent.

C. Was there evidence of electron transfer from the anode to the cathode? Use your data in Data Table 2 to explain your answer.

D. For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half reaction, and calculate the standard cell potential of the reaction. Use Table 1 in the Background as needed. Explain how you identified which half-reaction is the oxidizer and which is the reducer. Show all of your work.

Redox reaction: Cu(s) + Fe⁺³(aq) → Cu²⁺ (aq) + Fe²⁺ (s)