Question

Ag(s)+CN−(aq)+O2(g)→Ag(CN)−2(aq) Express your answer as a chemical equation. Identify all of the phases in your answer. Express your answer as a chemical equation. Identify all of the phases in your answer. Express your answer as a chemical equation. Identify all of the phases in your answer.

Answer 1

Answer : The balanced redox reaction will be,

$4Ag(s)+8CN^-(aq)+O_2(g)+4H^+(aq)\rightarrow 4Ag(CN)_2^-(aq)+2H_2O(l)$

Explanation :

The given chemical equation is,

$Ag(s)+CN^-(aq)+O_2(g)\rightarrow Ag(CN)_2^-(aq)$

In the half reaction method, the number of atoms in each half reaction and number of electrons must be balanced.

The half reactions in the acidic medium are :

Reduction : $O_2(g)+4H^+(aq)+4e^-\rightarrow 2H_2O(l)$   ......(1)

Oxidation : $Ag(s)+2CN^-(aq)\rightarrow Ag(CN)_2^-(aq)+1e^-$  .......(2)

Now multiply the equation (2) by 4 and then added both equation, we get the balanced redox reaction.

Thus, the balanced redox reaction will be,

$4Ag(s)+8CN^-(aq)+O_2(g)+4H^+(aq)\rightarrow 4Ag(CN)_2^-(aq)+2H_2O(l)$