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Wilfrid Laurier University CH Fundamentals of Chemistry II_Experiment 6: Electrochemistry: Voltaic Cells, Electrolysis and Faraday’s Law

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CH Fundamentals of Chemistry II_Experiment 6

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CH Fundamentals Of Chemistry II_Experiment 6

Experiment 6: Electrochemistry: Voltaic Cells, Electrolysis and Faraday’s Law Name: Sarah Bradburn Student #: Date Conducted: March 20th, 2017 Date Submitted: March 27th, 2017 Partner ’s Name: Sharif Kamal Lab Section: Monday 7:00, Section 3 IA’s Name: Sidney Nabuurs Abstract The purpose of ...

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ch fundamentals of chemistry iiexperiment 6
wilfrid laurier university ch fundamentals of chemistry iiexperiment 6
wilfrid laurier university ch fundamentals of chemistry iiexperiment 6 electroch

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Experiment 6: Electrochemistry: Voltaic Cells, Electrolysis and Faraday’s Law
Name: Sarah Bradburn
Student #: 160749140
Date Conducted: March 20th, 2017
Date Submitted: March 27th, 2017
Partner’s Name: Sharif Kamal
Lab Section: Monday 7:00, Section 3
IA’s Name: Sidney Nabuurs
Abstract
The purpose of this lab was to find the experimental equivalent weight of zinc and copper
and compare it to their theoretical equivalent weights. This was done by the construction of a
Voltaic Cell that conducted two electrolysis processes one with two copper electrodes and the
other with two zinc electrodes. The amount of total charge in micro amps was obtained from an
ammeter over an hour period of time. The electrodes were weighted on an analytical balance
before and after the electrolysis processes. The two copper electrodes had a difference weight of
0.0305 g and -0.0298 g. The two zinc electrodes had a difference weight of -0.0335 g and 0.0301
g. The total charge transferred over the system was 91.5 C. The experimental equivalent weight
of copper was 32.07 g. The experimental valence of the copper was 1.98 which had a 1% error
compared to the theoretical valence which was 2. For zinc the experimental equivalent weight
was 33.54 g. This was not so successful the percentage difference between the expected value of
2 valence and experimental value of 1.95 valence had a difference of 2.5%. At the end of this
experiment it was concluded that it was successful.
Procedure
For the procedure, refer to lab manual (CH111 Lab Manual, Winter 2017) pages 88-90.
Wilfrid Laurier University Chemistry Department. Winter 2017.Electrochemistry: Voltaic
Cells, Electrolysis and Faraday’s Law. Pages 88-90 in Chemistry 111 Laboratory Manual. Wilfrid
Laurier University, ON, Canada.
Results
Table 1: Qualitative Observations
Substance Observation
CuSO4 Dark blue, transparent liquid
ZnSO4 Colourless, transparent liquid
Cu strip Copper/ brown, shiny, solid metal
Zn strip Silver, shiny, solid metal

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, Table 2: Quantitative Observations- Measured Current Throughout the Electrochemical
Reaction
Time Interval Reaction Interval Time Measured Average Charge
Time (min) (s) Current (mA) Current (mA) Transferred
(C)
#1 0 0 24.7 25.5 1.53
#2 1 60 26.3 26.4 1.58
#3 2 60 26.5 26.45 1.59
#4 3 60 26.4 26.35 3.16
#5 5 120 26.3 26.05 7.82
#6 10 300 25.8 25.75 7.73
#7 15 300 25.7 25.75 23.18
#8 30 900 25.8 25.3 22.77
#9 45 900 24.8 24.6 22.14
#10 60 900 24.4
Total Charge Transferred: 91.5 C
Table 3: Quantitative Observations- Mass of Cu and Zn strips
Copper: Anode Cathode (-) Zinc: Anode (+) Cathode (-)
(+)
Initial Mass (g) 13.2897 11.2046 2.8090 2.0941
Final Mass (g) 13.3202 11.1748 2.8391 2.0606
Difference (g) 0.0305 -0.0298 0.0301 -0.0335
Discussion
Calculations
1. #Faradays= total charge/ F
#Faradays= 91.5 C/ 96485 C/mol
#Faradays= 9.48×10-4 mol
2. Equivalent Weight= (|Cu cathode| + |Cu anode|)/2/ # of equivalents
Equivalent Weight= (|-0.0298| + |0.0305|)/2/ 9.48×10-4
= 32.07 g
Valence= atomic weight/ calculated equivalent weight
Valence= 63.55 g/ 32.07g
Valence= 1.98
Expected Valence= atomic weight/ expected equivalent weight
= 63.55 g/ 31.78 g
=2
Percentage Difference= (|experimental – expected|/ expected) ×100%
= (|1.98 – 2|/ 2) ×100%
= 1%

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Exam (elaborations)

Wilfrid Laurier University CH Fundamentals of Chemistry II_Experiment 6: Electrochemistry: Voltaic Cells, Electrolysis and Faraday’s Law

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