Two electrolytic cells are connected in series and the same current passes through each cell. The first cell contains silver electrodes in silver nitrate solution. The second cell contains copper electrodes in copper(II) sulfate solution. In one experiment 1.00 g of silver is deposited in the first cell. What mass of copper, in g, is deposited in the second cell?

A.     \(\frac{{1.00}}{{107.87}}\)

B.     \(\frac{{1.00}}{{63.55}}\)

C.     \(\frac{{1.00}}{{107.87}} \times \frac{{63.55}}{2}\)

D.     \(\frac{{1.00}}{{107.87}} \times 63.55\)

C

One respondent stated that mentioning the fact that the same current passes through each cell may have been better than using the term in series. This is a fair point. The question overall was reasonably challenging with 53.53% of candidates getting the correct answer, C.