Project Report

Project Report

Submitted

On

Class – XII

Submitted To: Submitted By:

Mr. Sunil Jangda Pankaj Gill
Dept. of Chemistry Class – XII

1
 Certificate
This is to certify that Pankaj Gill,
Gill student of Class XII , Mahendra Model Sr. Sec.
School has completed the project titled Variation of Conductance with Temperature
in Electrolytes during the academic year 2009-2010 towards partial fulfillment of credit
for the Chemistry practical evaluation of CBSE 2010, and submitted satisfactory
report, as compiled in the following pages, under my supervision.

Mr. Sunil Jangra

Department of Chemistry
Mahendra Model Sr. Sr. School

2
 Acknowledgements

"There are times when silence speaks so much more loudly than words of praise to
only as good as belittle a person, whose words do not express, but only put a veneer
over true feelings, which are of gratitude at this point of time."

I would like to express my sincere gratitude to my chemistry mentor Mr. Sunil Jangra
, for her vital support, guidance and encouragement - without which this project
would not have come forth. I would also like to express my gratitude to the staff of the
Department of Chemistry at Mahendra Model Sr. Sec. School for their support during
the making of this project.

(Pankaj Gill)

3
 Index

1. Aim 5
2. Apparatus 6
3. Important Terms 7
4. Conductivity 8
5. Factors Affecting Electrical Conductivity 9
6. Procedure 10
7. Physical Constants 11
8. Observation Set 1 12
9. Graph of Observation Set 1 13
10. Observation Set 2 14
11. Graph of Observation Set 2 15
12. Result 16
13. Conclusion 17
14. Precautions 18
15. Bibliography 19

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 Aim

To find the variation of conductance with temperature in

electrolytes

5
 Apparatus

Glass beaker, CuSO4 solution, Cu electrodes, ZnSO4 solution, Zn

electrodes, rheostat, battery eliminator, water, burner,
thermometer, flask, ammeter, voltmeter

6
 Important Terms

Conductance: The property of ease of flow of electric
current through a body is called conductance.

Resistance: The obstacle offered to the flow of electric

current is called resistance.

Electrolysis: The operation in which electricity causes a

chemical reaction is called electrolysis.

Ohm's Law: This law states that the current flowing

through a resistance is directly proportional to the potential
difference applied across it's ends, at constant temperature
and pressure.
V=IxR

Faraday's Laws:

First Law: The mass of a substance produced or
consumed in electrolysis is directly proportional to the
quantity of charge passing through it.
m Q
or, m = Z × I × t
where, Z is electrochemical equivalent; I is current; t is
time in seconds; Q is charge.

Second Law: The mass of substance produced in

electrolysis directly proportional to its equivalent mass.
W1 / E1 = W2 / E2 = W3 / E3...

Third Law: The mass of a substance produced in

electrolysis is directly proportional to the number of
electrons per mole needed to cause desired change in
oxidation state.

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 Conductivity

When voltage is applied to the electrodes immersed into an

electrolyte solution, ions of electrolyte move, and thus, electric
current flows through the electrolytic solution. The electrolytic
solution and the metal conductors exhibit resistance to the
passage of the current; both of which obey Ohm's law.

The reciprocal of resistance is called electrical conductance. The

unit of electrical conductance is Siemens (S) or ohm-1 or mho.

If a solution is placed between two parallel electrodes having

cross sectional area A and distance L apart then the resistance is
given by

R=1/C

ρ (called 'rho') is known as resistivity. Its reciprocal gives the

conductivity of the solution, which is denoted by κ (called
'kappa'). Its unit is Siemens/meter.

Κ=1/R*L/A

L / A is a fixed quantity for a cell and is called the 'cell constant'.

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 Factors Affecting Electrical
Conductivity

The factors which affect the electrical conductivity of the

solutions are:

Inter-ionic attraction: It depends on solute- solute

interactions.

Solvation of ions: It depends on solute-solvent
interactions.

Viscosity of the solvent: It depends on solvent-solvent
interactions.

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 Procedure

1. The electrolyte chosen is ZnSO4 and the electrodes are of

Zn.
2. Readings for the measurement of conductance are taken at
intervals of 3 ⁰C.
3. Proper precautions are taken to avoid evaporation and to
keep other factors constant.
4. The vessel and electrodes are removed and the vessel is
cleaned and filled with ZnSO4 solution.
5. The electrodes are refitted in their original place so that
the distance between them does not change.
6. Current is passed and when the voltmeter and ammeter
show steady readings, they are noted.
7. The current is switched off.
8. It is seen that while the ammeter reading returns at once to
0 position. The voltmeter needle pauses for a while at a
particular reading which is noted down.
9. This reading indicates the back EMF in the electrolyte.
10.Similarly, more sets of reading are taken, and resistance is
calculated.
11.Thus, the value of conductance is calculated.
12.The switched on circuit readings in voltmeter and ammeter
are taken.
13.The current through the electrolyte is changed by adjusting
the rheostat and more sets of readings are taken.
14.Thus, the mean value of resistance is calculated.
15.Above steps are repeated for CuSO4 as electrolyte with
electrodes made of Cu.

10
 Physical Constants

For the purpose of accuracy and convenience, some important

aspects of the electrolyte process are kept constant in the
experiment as their variation might affect the conductivity of the
electrolyte. They are:

Voltage

Nature of electrodes

Size of electrodes

Separation between the electrodes

Concentration of the electrolytes

Nature of the electrolytes

Resistance in the circuit

11
 Observation Set 1
For ZnSO4 electrolyte with Zn electrodes

S Temperature Reading Reading Resistance Conductance

No of of
Ammeter Voltmeter

I V R=V/I C=1/R
1 23 ⁰C 100 mA 1.0 V 10 Ω 0.100 Ω-1
2 26 ⁰C 100 mA 0.95 V 9.5 Ω 0.105 Ω-1
3 29 ⁰C 110 mA 0.89 V 8.09 Ω 0.120 Ω-1
4 32 ⁰C 110 mA 0.84 V 7.63 Ω 0.130 Ω-1
5 35 ⁰C 120 mA 0.80 V 6.66 Ω 0.150 Ω-1
6 38 ⁰C 125 mA 0.75 V 6.00 Ω 0.160 Ω-1
7 41 ⁰C 130 mA 0.71 V 7.6 Ω 0.180 Ω-1
8 44 ⁰C 130 mA 0.65 V 5.00 Ω 0.200 Ω-1

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 Graph of Observation Set 1

Zinc Sulphate Electrolyte

0.25

0.2
0.2
Conductance (in Mho)

0.18

0.16
0.15
0.15
0.13
0.12

0.11
0.1
0.1

0.05

0
20 25 30 35 40 45 50
Temperature (in degree Celsius)

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 Observation Set 2
For CuSO4 electrolyte

S Temperature Reading Reading of Resistance Conductance

No of Voltmeter
Ammeter

I V R=V/I C = 1/R
1 25 ⁰C 75 mA 1.4 V 18.67 Ω 0.053 Ω-1
2 28 ⁰C 75 mA 1.35 V 18.00 Ω 0.055 Ω-1
3 31 ⁰C 75 mA 1.3 V 17.33 Ω 0.057 Ω-1
4 34 ⁰C 75 mA 1.25 V 16.67 Ω 0.060 Ω-1
5 36 ⁰C 80 mA 1.2 V 15.00 Ω 0.066 Ω-1
6 38 ⁰C 80 mA 1.15 V 14.38 Ω 0.069 Ω-1
7 42 ⁰C 80 mA 1.10 V 13.75 Ω 0.072 Ω-1
8 44 ⁰C 85 mA 1.10 V 12.94 Ω 0.075 Ω-1
9 47 ⁰C 85 mA 1.05 V 12.35 Ω 0.080 Ω-1
10 49 ⁰C 90 mA 1.10 V 11.11 Ω 0.090 Ω-1
11 53 °C 90 mA 1.90 V 10.00 Ω 0.100 Ω-1

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 Graph of Observation Set 2

Copper Sulphate Electrolyte

0.12

0.1
0.1
0.09

0.08
0.08 0.08
0.07
Conductance (in Mho)

0.07
0.07

0.06
0.06 0.06
0.06
0.05

0.04

0.02

0
20 25 30 35 40 45 50 55
Temperature (in degree Celsius)

15
 Result

The relevant graph shows that the 1 / Resistance of an

electrolyte increases at a steady rate as the temperature
increases.

16
 Conclusion

On heating a solution, it is known that viscosity gradually

decreases, with decrease in viscosity, the speed and movement
of the ions increases. In other words, the conductance of the
electrolyte increases with increases in temperature. Hence, the
result of the experiment agrees with reasoning.

17
 Precautions

Variation of resistance due to one of the factors should be

kept constant.

The electrodes used in each case should always be kept
parallel to each other.

The solution should be kept undisturbed throughout the
experiment.

For each observation, three readings are taken and the
mean value is considered.

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 Bibliography

Chemistry (Part I) – Textbook for Class XII; National

Council of Educational Research and Training

Pardeep’s Fundamental of Chemistry for Class

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