Question

Consider a battery with the overall reaction: Cu(s) + 2Ag+(aq) ⟶ 2Ag(s) + Cu²+(aq).

If a particular dead battery was found to have [Cu²+] = 0.11M, what was the concentration of silver ion?

Answer 1

In the given redox reaction, the stoichiometric coefficient indicates that the concentration of Ag+ ions is twice that of Cu²+ ions. Therefore, if the concentration of Cu²+ is 0.11M, the concentration of Ag+ ions would be 0.22M.

Step-by-step explanation:

The question deals with the concept of stoichiometry in redox reactions. In the equation Cu(s) + 2Ag+⟶ 2Ag + Cu²+, the stoichiometric coefficient before Ag+ is '2', which means for every one Cu²+, two Ag+ ions react. Hence, the concentration of Ag+ ions is twice that of Cu²+. Given [Cu²+] = 0.11M, using the stoichiometric relationship, we can find the concentration of Ag+ ions. Hence, [Ag+] = 2*[Cu²+] = 2*0.11M = 0.22M.

Learn more about Redox Reactions