When a solution of nickel(II) sulfate adjusted to a pH of 7 is electrolyzed, the

Question

When a solution of nickel(II) sulfate adjusted to a pH of 7 is electrolyzed, the green color of the solution becomes intense in the cathodic chamber and gas bubbles are detected in the anodic chamber. (0) Write a balanced equation for the half-reaction occurring at the anode. 01 (ii) Write a balanced equation for the half-reaction occurring at the cathode. Data for the experimental determination of Avogadro's Number and the Paraday Constant (See Re correct number of significant figures. are recorded for Trial 1 port Sheet.) in the table. Complete the analysis for those determinations. Record the calculated values with the B. Determination of Avogadro's Number and the Faraday Constant 1. Initial mass of copper anode (mL) 4. Time of electrolysis (s) 5. Current (or average current) (A,C) 6. Final mass of copper anode (g) 24852 Data Analysis 2. 2.1335 Data Analysis 3 Data Analysis 1. Mass of copper oxidized at anode (g) 2. Moles of copper oxidized (mol) Data Analysis 4 Show caculation. 3. Moles of electrons transferred (mol e" Equation 33.4 Show calculation. Data Analysis 5 4. Coulombs passed through cell (C) Equation 33.5. Show calculation. 5. Electrons passed through cell (e) Data Analysis 6. Equation 33.6 Show calculation. 6. Avogadro's number (e /mol e) Equation 33.7 Show calculation. 9. Percent error Data Analysis 10. 10. Faraday constant(C/mol e) Equation 33.8 Show caleulation.

Explanation / Answer

Q1.

mass of copper oxidized at anode = Initial - Final mass = 2.4852-2.1335 = 0.3517 g oxidized

Q2.

moles of copper = mass/MW = 0.3517/63.5 = 0.005538 mol of Cu

Q3

moles of e- transferrec

if Cu(s) = Cu+2 + 2e-

then

0.005538 mol of Cu = 2*0.005538 mol of e- = 0.011076 mol of e-

Q4

C = I*t

C= 0.622*1702

C = 1058.644 C

Q5.

charge of e- = 1058.644

x e- = 1058.644 *10^-19

e = (1058.644 )/(1058.644 *10^-19) = 10^19 e-

Q6.

A = e- / mol of e- = ( 10^19) / (0.011076 ) = 9.02*10^20

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