write a balanced net ionic equation for the overall reaction represented by the cell notation below.
Pt/ Fe2+, Fe3+ // I-/AgI/Ag
oxidation: Fe2+ --> Fe3+ + e-
Reduction: Ag+ +e --> Ag
overall is;
Fe2+ + Ag+ --> Fe3+ + Ag
write a balance net ionic equation for the overall reaction represented by the following cell notation. Al(s) | Al3+(aq) || Cl2(g) | Cl^-(aq) | Pt(s)
Al + Cl- = Al3+ + Cl2
To write a balanced net ionic equation for the overall reaction represented by the given cell notation, we need to first understand the individual components of the cell notation and their corresponding reactions.
Pt represents a platinum electrode, which is inert and doesn't participate in the reaction.
Fe2+, Fe3+ represents a redox couple involving iron ions in two different oxidation states. The oxidation half-reaction involves Fe2+ losing electrons to form Fe3+, while the reduction half-reaction involves Fe3+ gaining electrons to form Fe2+.
I-/AgI/Ag represents another redox couple involving iodide ions and silver. The oxidation half-reaction involves iodide ions losing electrons to form elemental iodine (I2), while the reduction half-reaction involves silver ions gaining electrons to form elemental silver (Ag).
To obtain the net ionic equation, we need to identify the species that are directly involved in the reaction and the corresponding balanced reactions.
For Fe2+/Fe3+:
Fe2+ (aq) → Fe3+ (aq) + e- (Oxidation half-reaction)
Fe3+ (aq) + e- → Fe2+ (aq) (Reduction half-reaction)
For I-/AgI/Ag:
2 I- (aq) → I2 (s) + 2 e- (Oxidation half-reaction)
2 Ag+ (aq) + 2 e- → 2 Ag (s) (Reduction half-reaction)
Now, we will create the overall balanced net ionic equation by combining the two balanced half-reactions:
Fe2+ (aq) + 2 I- (aq) → Fe3+ (aq) + I2 (s) (Overall net ionic equation)
Therefore, the balanced net ionic equation for the overall reaction represented by the given cell notation is:
Fe2+ (aq) + 2 I- (aq) → Fe3+ (aq) + I2 (s)