what is the net ionic equation for FeSO4 + KCl = FeCl2 + K2SO4?
To determine the net ionic equation for the given reaction, we first need to write the balanced molecular equation.
The given starting reactants are FeSO4 (iron(II) sulfate) and KCl (potassium chloride), and the products are FeCl2 (iron(II) chloride) and K2SO4 (potassium sulfate).
The balanced molecular equation for this reaction is:
FeSO4 + 2KCl → FeCl2 + K2SO4
To find the net ionic equation, we need to identify the ions that are directly involved in the reaction and eliminate the spectator ions. Spectator ions are ions that are present on both sides of the equation but do not undergo any changes.
In this case, the complete ionic equation is:
Fe^2+ (aq) + SO4^2- (aq) + 2K^+ (aq) + 2Cl^- (aq) → Fe^2+ (aq) + 2Cl^- (aq) + 2K^+ (aq) + SO4^2- (aq)
Since Fe^2+ and 2Cl^- are present on both sides of the equation as spectator ions, we can eliminate them:
SO4^2- (aq) + 2K^+ (aq) → K2SO4 (aq)
This is our net ionic equation. It shows the actual species involved in the reaction, excluding the spectator ions. Therefore, the net ionic equation for FeSO4 + KCl = FeCl2 + K2SO4 is:
SO4^2- (aq) + 2K^+ (aq) → K2SO4 (aq)
To write the net ionic equation for the given reaction, we first need to write the balanced chemical equation:
FeSO₄ + 2KCl → FeCl₂ + K₂SO₄
Now, let's break down the equation into its respective ions:
Fe²⁺ + SO₄²⁻ + 2K⁺ + 2Cl⁻ → Fe²⁺ + 2Cl⁻ + 2K⁺ + SO₄²⁻
As we can see, the Fe²⁺ and SO₄²⁻ ions appear on both sides of the equation and do not participate in the overall reaction. These ions are considered spectator ions. Therefore, the net ionic equation can be written by removing the spectator ions:
Net Ionic Equation: SO₄²⁻ + 2K⁺ → 2K⁺ + SO₄²⁻
Simplifying this equation, we can conclude that there is no net change in the reaction as all ions remain the same on both sides. Thus, the net ionic equation for the given reaction is:
Net Ionic Equation: No reaction takes place