What weight of lead sulfate is produced during discharge of a lead storage battery over a 3.0 hour period at an average current of 0.50 amp? [Hint: Consider both electrode processes.]
A) 8.6 g
B) 17 g
C) 26 g
D) 53 g
E) 61 g

Question

Quizplus · Accepted Answer

The reaction at both electrodes involves the formation of PbSO4. The total charge passed is calculated using Q = It = 0.50 A * 3.0 h * 3600 s/h = 5400 C. The number of moles of electrons is Q/F = 5400 C / 96485 C/mol = 0.056 mol. Since 2 moles of electrons produce 1 mole of PbSO4, the moles of PbSO4 formed is 0.056 mol / 2 = 0.028 mol. The molar mass of PbSO4 is 303 g/mol, so the mass is 0.028 mol * 303 g/mol = 8.484 g, which is approximately 17 g when considering both electrodes.

What Weight of Lead Sulfate Is Produced During Discharge of a Lead