Final answer:
To determine the coulombs of electricity used to produce 6.84 g of tin from molten SnSO4, the number of moles of tin is calculated, then the charge in coulombs based on the moles of electrons required for the reaction is determined, yielding a total of 11,117 coulombs.
Step-by-step explanation:
To calculate the coulombs of electricity used to produce 6.84 g of metallic tin, we need to apply Faraday's laws of electrolysis and stoichiometry. The reaction for the reduction of tin from tin(II) sulfate (SnSO4) in the molten state to tin metal (Sn) is as follows:
Sn2+ (l) + 2e- → Sn (s)
According to the reaction, 1 mol of Sn2+ requires 2 moles of electrons to be reduced to metallic tin. We first calculate the moles of tin:
Molar mass of Sn = 118.71 g/mol
Moles of Sn = Mass of Sn / Molar mass of Sn
Next, we calculate the moles of electrons required to produce this amount of Sn:
One mole of electrons equals 96,485 C (1 Faraday). Therefore, the total charge (Q) required is:
Q = Moles of electrons * Charge of 1 mol of electrons
Thus, 11,117 coulombs of electricity were used to produce 6.84 g of metallic tin from molten SnSO4.