# Experimental Verification

To verify the Faraday’s first law of electrolysis, experimental arrangement is shown in figure.

To verify the current, the different magnitude of current is passed through the copper sulphate solution with the help of Rheostat in equal interval of time. At that time, masses of ions deposited or liberated on an electrode is calculated. If m1, m2 and m3 are the masses of ions deposited or liberated on an electrode for currents I1, I2 and I3, respectively, then it’s found that,

m1 / I1 = m2 / I2 = m3 / I3 = constant

i.e. m/I = constant

i.e. m ∝ I ——– (i)

To verify the time period, same magnitude of current is passed through the electrolyte in different interval of time. At that time, masses of ions deposited or liberated on an electrode is noted.

If m1, m2 and m3 are the masses of ions deposited or liberated on an electrode for time periods t1, t2 and t3, respectively, then it’s found that,

m1 / t1 = m2 / t2 = m3 / t3 = constant

i.e. m / t = constant

i.e. m ∝ t ——– (ii)

Combining equations (i) and (ii), We get,

m ∝ I t

∴ m ∝ q

To verify the Faraday’s second law of electrolysis, experimental arrangement is shown in figure.

3 voltameters; Cu, Zn and Ag are connected in series and same magnitude of current is passed through the electrolytes. At that time, masses of ions deposited on different voltameters are noted. If mCu, mZn and mAg are the masses of ions deposited or liberated on an electrode for Cu, Zn and Ag and their respective chemical equivalence are ECu, EZn and EAg, then it’s found that,

mCu / ECu = mZn / EZn = mAg / EAg

i.e. m / E = constant

i.e. m ∝ E