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To determine the value of Faraday constant (quantity of electricity per mole) by using electrolysis of Copper.

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  • Essay length: 841 words
  • Submitted: 31/03/2006
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1) Title:

QN1 A Quantitative study of electrolysis

2) Aim/Objective:

To determine the value of Faraday constant (quantity of electricity per mole) by using electrolysis of Copper.

3) Results:

Before electrolysis:

Weight of cathode = 2.164 g

Weight of anode = 2.502 g

After electrolysis:

Weight of cathode = 2.237 g

Weight of anode = 2.435 g

Time of electrolysis = 20 minutes

= 1200 seconds

Ammeter reading = 0.19A

4) Calculation/interpretation:

The equation of the electrolysis reaction at the cathode:

Cu2+(aq.) + 2e- Cu(s.)

Gain in weight of cathode = 2.237g - 2.164g

= 0.073 g

Loss in weight of anode = 2.520 - 2.435g

= 0.085 g

No. of moles of loss in cupper anode = 0.085 / 63.5

= 0.00134 mol

Quantity of electricity required = 0.00134 mol * 2

= 0.00268 mol

Quantity of electricity supplied = 1200 * 0.19

= 228C

Faraday Constant = quantity of electricity / no.

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