the information below describes a redox reaction.\nag⁺(aq) + al(s) → ag(s) + al³⁺(aq)\nag⁺(aq) + e⁻ →…
the information below describes a redox reaction.\nag⁺(aq) + al(s) → ag(s) + al³⁺(aq)\nag⁺(aq) + e⁻ → ag(s)\nal(s) → al³⁺(aq) + 3e⁻\nwhat is the coefficient of silver in the final, balanced equation for this reaction?\no 1\no 2\no 3\no 4
Answer
Explanation:
Step1: Balance the electrons
The reduction half - reaction is $Ag^+(aq)+e^-\rightarrow Ag(s)$ and the oxidation half - reaction is $Al(s)\rightarrow Al^{3 +}(aq)+3e^-$. To balance the electrons, we multiply the reduction half - reaction by 3 so that the number of electrons lost in oxidation equals the number of electrons gained in reduction. $3Ag^+(aq)+3e^-\rightarrow 3Ag(s)$ and $Al(s)\rightarrow Al^{3 +}(aq)+3e^-$
Step2: Combine the half - reactions
Combining the two half - reactions gives $3Ag^+(aq)+Al(s)\rightarrow 3Ag(s)+Al^{3 +}(aq)$
Answer:
3