Data for the experimental determination of Avogadro\'s Number and the Faraday Co

Question

Data for the experimental determination of Avogadro's Number and the Faraday Constant are recorded for Trial 1 (Sec Report Sheet.) in the table. Complete the analysis for those determinations. Record the calculated values with the correct number of significant figures. Initial mass of copper anode (mL) Time of electrolysis (s) Current (or average current) (A, C/s) Final mass of copper anode (g) Mass of copper oxidized at anode (g) Moles of copper oxidized (mol) Show calculation Moles of electrons transferred (mol e^-) Equation 33.4. Show calculation. Coulombs passed through cell (e^-) Equation 33.5 Show calculation Electrons passed through cell (e^-) Equation 33.6 Show calculation Avogadro's number (e^-l/mol e^-) Equation 33.7 Show calculation. Percent error Faraday constant (C/mol e^-) Equation 33.8 Show calculation.

Explanation / Answer

From the given data

1. mass of Cu oxidized = 2.4852 - 2.1335 = 0.3517 g

2. moles of Cu = 0.3517 g/63.546 g/mol = 0.00553 mol

3. moles of e- transferred = 0.00553 x 2 = 0.01106 mol e-

4. coulombs passed = I x t = 0.622 x 1702 = 1058.644 C

5. Electrons passed = 1058.644/1.602 x 10^-19 = 6.61 x 10^21 e-

6. Avogadro's number = 6.61 x 10^21/0.01106 = 5.98 x 10^23

7. Percent error = (6.023 x 10^23 - 5.98 x 10^23) x 100/6.023 x 10^23 = 0.714%

8. Faraday's constant = 1058.644/0.01106 = 95718.264

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