Two cells are connected in series, so that the same current flows through two electrodes where the following half-reactions occur Cu²⁺(aq) + 2e^- → Cu(s) and Ag⁺(aq) + e_- → Ag(s)
For every 1.00 g of copper produced in the first process, how many grams of silver will be
Produced in the second one?

Question

Quizplus · Accepted Answer

The molar mass of Cu is 63.55 g/mol and Ag is 107.87 g/mol. For every mole of Cu produced, 2 moles of electrons are used, and for every mole of Ag produced, 1 mole of electrons is used. Therefore, for 1 g of Cu (1/63.55 moles), 2/63.55 moles of electrons are used, which will produce 2/63.55 moles of Ag. This corresponds to (2/63.55) * 107.87 g of Ag, which is approximately 3.40 g.

Two Cells Are Connected in Series, So That the Same