Question

Examine each of the following pairs of potential reactants. Decide whether or not a reaction would occur. If a reaction occurs, write the balanced equation. If no reaction occurs, write NR. Fluorine and potassium iodide

Answer 1

Using the activity series, we find that fluorine will displace iodine in a single-replacement reaction with potassium iodide, resulting in potassium fluoride and solid iodine. The balanced chemical equation is 2 F₂ (g) + 2KI (aq) → 2 KF (aq) + I₂ (s).

Step-by-step explanation:

The question examines whether a reaction occurs when fluorine as a reactant and potassium iodide. When considering single-replacement reactions in this context, we look at the activity series of halogens, which tells us that a halogen can replace another halogen in a compound if it is higher in the group on the periodic table. Because fluorine is above iodine in the periodic table, it is more reactive and can displace iodine from its compounds. The reaction that occurs is:

2 F₂ (g) + 2KI (aq) → 2 KF (aq) + I₂ (s)

Here, fluorine replaces iodine in potassium iodide to form potassium fluoride and solid iodine. This is a redox reaction where fluorine is reduced and iodine is oxidized. The equation above is already balanced. If the activity of the halogen was not sufficient to replace the other, then we would write NR (no reaction).