Main Introduction Initial Observation and Hypothesis Materials and Equipment Experiment Discussion Applications Conclusions

DISCUSSION

Data Analysis

The experimental results are presented on the charts below.

The graphs show that the measurements taken for 3-V voltage are closer together than the measurements taken for 1.5-V voltage. This happens because the lower voltage generates lower current; the lower the current the greater the error of measurements. Therefore the larger discrepancy observed at 1.5 V is caused by the larger value of the error in the measurements.

The graphs also show a larger discrepancy for higher concentrations of salt. We think this occurs because when the concentration of salt is higher the salt doesn’t dissolves in the water completely. As a result, the solution is not perfectly homogenous, which causes the discrepancy.

Theory

Faraday’s Laws of Electrolysis can be expressed by the mathematical equation:

Where:

m is a mass deposited as metal or evolved as gas

F is called Faraday’s constant and equals 9.65 x 10⁴ C mol^-1

I is a current occurring through the solution

t is a time

A is a molar mass of the metal or gas

n is the number of electrons required to produce the ion from the given substance; for salt/water solution n = 2

It is reasonable to suggest that the mass deposited on the electrodes increases with the concentration of salt. Since the mass is proportional to the current, we can mathematically state that the current increases with the concentration of the salt.

Therefore our experimental results are in good agreement with the theory.