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Tindoy Exp.6

This document describes an experiment using an online simulation of a voltaic cell to measure voltage generated by different combinations of metal electrodes and ionic solutions. The student sets up combinations of silver/copper in silver nitrate or copper nitrate solutions, observing a voltage of +0.46 V from copper to silver. Additional combinations tested include silver or copper in zinc nitrate or hydrogen chloride solutions, recording the voltages and direction of electron flow for each.

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Khrisha Tindoy
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132 views3 pages

Tindoy Exp.6

This document describes an experiment using an online simulation of a voltaic cell to measure voltage generated by different combinations of metal electrodes and ionic solutions. The student sets up combinations of silver/copper in silver nitrate or copper nitrate solutions, observing a voltage of +0.46 V from copper to silver. Additional combinations tested include silver or copper in zinc nitrate or hydrogen chloride solutions, recording the voltages and direction of electron flow for each.

Uploaded by

Khrisha Tindoy
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
Available Formats
Download as PDF, TXT or read online on Scribd
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Experiment No.

6
Voltaic Cells

Name: Tindoy, Khrisha Mae V. Course/Section: BETET NS 2A


I. Data Collection:

A. Go to http://introchem.chem.okstate.edu/DCICLA/voltaicCell20.html and open the


Voltaic Cells Simulation. Your screen should look like the figure.

This simulation contains an apparatus for measuring the voltage generated by chemical reactions.
This apparatus is called a voltaic cell. Pop out menus will allow you to select metals (electrodes)
and ionic solutions to be placed into two beakers that are connected by a salt bridge. You can then
connect the metals to a voltmeter to measure the cell voltage (Eº).

Simulation: https://chemdemos.uoregon.edu/demos/Electrochemical-Cells-Computer
Simulation-Voltaic-Cells-Zn-Cu-Ag 1
B. Click on the left pop-out tab for metals and select silver. Click on the left pop-out tab for
solutions and select AgNO3 (aq). Use the right tabs and select Cu and Cu(NO3)2 (aq). Click on the
power switch of the voltage meter. Observe the action of the simulation. Use the following
drawing to sketch and label what is happening and to answer the following questions.

What is the voltage (Eº) generated by the chemical reaction?


- The voltage generated by the chemical reaction is +0.46 V

What direction are the electrons flowing?


- The direction of the electrons are from right to left.

II. Data Analysis and Interpretation

A. What happens to the electrons that are on to the Ag metal electrode?


- The electrons that are on to the Ag metal electrode are consumed.

B. What happens to the electrons that are on to the Cu metal electrode?


- The electrons that are on to the Cu metal electrode stays on the solution.

Simulation: https://chemdemos.uoregon.edu/demos/Electrochemical-Cells-Computer
Simulation-Voltaic-Cells-Zn-Cu-Ag 2
C. Write a net ionic equation representing what is happening in the left beaker. (This is
called a half reaction.)
- AgNO3

D. Write a net ionic equation representing what is happening in the right beaker. (This is
called a half reaction.)
- Cu(NO3)2

E. Combine the two half reactions into a complete reaction.


- AgNO3 + Cu(NO3)2 → Ag(NO3)2

F. Determine what happens if you reverse the cell by placing the Ag/AgNO3 system in the
right beaker and the Cu/Cu(NO3)2 system in the left beaker. Explain what you observe.
- The voltage changes from positive to negative, thus the voltage is -0.46 V.
The direction of the electrons changes from right to left to left to right.

III. Data Collection:

Repeat the procedure of section I. for all the combinations in the following table.
Record the cell voltages for each condition. Record the direction of electron flow
from electrode to electrode.

Left Cell Right Cell Voltage (Eº) Direction of Electrons


/Spontaneous
Ag/AgNO3 Cu/Cu(NO3)2 + 0.46 From Cu to Ag
Ag/AgNO3 Zn/Zn(NO3)2 +1.56 From Zn to Ag
Ag/AgNO3 H2/HCl +0.80 From HCl to Ag
Cu/Cu(NO3)2 Zn/Zn(NO3)2 +1.10 From Zn to Cu
Cu/Cu(NO3)2 H2/HCl +0.34 From HCl to Cu
Zn/Zn(NO3)2 H2/HCl -0.76 From Zn to HCl

Simulation: https://chemdemos.uoregon.edu/demos/Electrochemical-Cells-Computer
Simulation-Voltaic-Cells-Zn-Cu-Ag 3

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