1. The document describes an experiment involving electrochemical and galvanic cells. It involves assembling half-cells of Cu2+ and Zn2+ solutions with copper and zinc electrodes, and measuring the voltage. 2. A galvanic cell is then assembled by connecting the half-cells with a salt bridge, and the voltage is measured for combinations of Zn/Zn2+, Cu/Cu2+, and Pb/Pb2+ electrode pairs. 3. The observed voltages are compared to theoretical standard electrode potentials to calculate percentage error. The document also discusses using fruit instead of a salt bridge and cautions against eating the fruit afterwards.

1. '
i_.
i·;'
j:
..·.·
.
·· ·. ;
·.
CHEM3 LAB. REPORT : .... :
: Expt#: _ Expt Title: Electrochemical & Galvanic Cells Date· Performed: - - - -
.Group#: __ Section: - - - - - Score: - - - - - - Date Submitted: - - - -
Objective:
Procedure:
A. L Add 0.5 M Cu(N03) 2 to the porous cup until it is about halffull. Plac~ a clean strip of copper in the I
cup. Connect the copper electrode to the positive terminalofthe voltmeter. I
2. Add 0.5 M Zn(N0 3)2 to the I SOml beaker until it is about 1/3 full. Place a clean strip of zinc in the f.
beaker. Connect the zinc electrode to the negative terminal of the voltmeter.
3. Note the voltage reading of the half cells.
4. Place the porous cup in the beaker. Note the voltage reading. Remove the porous cup and return all
the solutions and metal electrodes.
B. I. Assemble a galvanic cell by coupling 2 test electrodes. Dip one end of the salt bridge in one of the
half cells and the other end to the second half cell. The salt bridge is thread soaked in a supersaturated
/.
I KCI. The galvanic ells to be assembled involve the following pairs of electrodes:
• a) Zn/Zn 2+ electrode and Pb/Pb 2+ electrode
2+ 2+ .
b) Cu/Cu electrode and Zn/Zn electrode
~i c) Cu/Cu 2+ electrode and Pb/Pb 2+ electrode
.t
..... i 2. Connect each electrode to the input terminals of the voltmeter and read the voltage. If a negative
I voltage is observed, interchange the terminat'connections. Note the terminal to each electrode is
connected. The cathode is the half cell connected to the positive (red) terminal of the meter, and the
I
anode is the half cell connected to the negative (black) terminal. .
.
·
1:
Set-up: DRAW the set- up in part A and B
.'
i
i
·I
I
;
, .:
·;
Data:
Cell Observed E0 (V)
/1
I
a
b
c _ _I
I;
II
I .
!
J
..

2. 1," • •
' '. ; '
:CHEM 3 LAB. REPORT
;Questions:
.< :
Part A. _! ." ,
jt. Will the c~ll operate when arranged like the firstset-up (porous cup outside the beak~r)? Explain . .·.
..· .
I.
I
i
i
i
2. What is the purpose of the porous cup or salt bridge?
i
'
l '
.,
' ~
' : -~
3. What is the spontaneous half reaction taking place in the (i) Zn half cell and (ii) Cu hhlf cell ? Write the total
• . . I
1
react1on. 1 .,, .
'' ·!,.
I
I
I I '
4. What is the direction of electron flow in the wire connecting the zinc and copper electrodes? What is the
~irection ofthe flow of negative ions through the porous cup (or salt bridge)?
1
I '
I
I
l i
Part B.
l
i
,, I
I. Calculate the electromotive force (emt) of each galvanic cellassembled, using the s~andard electrode
potentials given below
Half reaction Eu (V) Cell Theoretical Eu (V)
.
zn:t+ + 2e- -7 Zn -0.763 a
Pb.l"' + 2e- -7 Pb -0.126 b
Cu.l"' + 2e· -7 Cu 0.337 c
..
'
2. Comtpare th e th eore. 1ca va ue WI'th th eo bserve d cOmQUte or o error
;
Cell %Error
I
I· a
b
c
~ *********************************
I
FOOD FORTHOUGHT . . . .
~ilnst~ad ofusing porous cup (or salt bridge) try using any citrus fruit, even banan~. Observe if a change in
potential will occur? WARNING: DO NOT EAT THE FRUIT THAT YOU'VE USED!!! .
~ .
·l!:l . .
... ·.·.,.' ::....
.
. ???
•. • •
.
. .
. .
. .·.
. .
i_l· ,· , ...
;~ J ' I
i'l
I
l .
,.
.
..
I