Two cells are connected in series, so that the same current flows through two electrodes where the following half-reactions occur Cu²⁺(aq) + 2e¯ $\rightarrow$ Cu(s) and Ag⁺(aq) + e¯ $\rightarrow$ 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

Two cells are connected in series, so that the same current flows through two electrodes where the following half-reactions occur Cu²⁺(aq) + 2e¯

\rightarrow

Cu(s) and Ag⁺(aq) + e¯

\rightarrow

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?

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 (2 electrons), 2 moles of Ag (2 electrons) are produced. Therefore, for 1 g of Cu, (1/63.55) moles of Cu are produced, which corresponds to (2 * 107.87/63.55) g of Ag, approximately 3.40 g.

Two Cells Are Connected in Series, So That the Same →\rightarrow→

Two Cells Are Connected in Series, So That the Same $\rightarrow$