What charge (in Coulombs)is required to oxidize 1.0 g of silver to silver(I)ions?
(F = 96480 C/mol e−)

Question

What charge (in Coulombs)is required to oxidize 1.0 g of silver to silver(I)ions? 
(F = 96480 C/mol e−)

Quizplus · Accepted Answer

To oxidize 1.0 g of silver to silver(I) ions, we need to calculate the charge required based on the molar mass of silver (Ag), which is approximately 107.87 g/mol, and the fact that the oxidation of silver to Ag+ involves the loss of one electron per atom of silver. The charge of one mole of electrons (Faraday's constant) is 96480 C/mol. First, calculate the moles of silver: $1.0 \, \text{g} \, \text{Ag} \times \frac{1 \, \text{mol} \, \text{Ag}}{107.87 \, \text{g} \, \text{Ag}} \approx 0.00928 \, \text{mol} \, \text{Ag}$.Then, calculate the charge required: $0.00928 \, \text{mol} \, \text{Ag} \times 96480 \, \text{C/mol} \, e^- \approx 8.9 \times 10^4 \, \text{C}$.This matches choice E.

What Charge (In Coulombs)is Required to Oxidize 1