what is the balanced formula equation, complete ionic equation, and net ionic equation FeSO4(aq) + KCl(aq)

First, you have been given a couple of salts that don't react.

FeSO4(aq) + KCl(aq) ==> no reaction.
FeSO4(aq) + KCl(aq) ==> Fe^+2(aq) + SO4^-2(aq) + K^+(aq) + Cl^-(aq)

FeSO4(aq) + 2KCl(aq) -> FeCl2(aq) + K2SO4(aq)

To form the complete ionic equation, we should break down all the compounds into their individual ions.

Fe2+(aq) + SO42-(aq) + 2K+(aq) + 2Cl-(aq) -> Fe2+(aq) + 2Cl-(aq) + 2K+(aq) + SO42-(aq)

In the net ionic equation, we cancel out any species that appear on both sides of the equation.

SO42-(aq) + 2K+(aq) -> 2K+(aq) + SO42-(aq)

Therefore, the balanced formula equation is FeSO4(aq) + 2KCl(aq) -> FeCl2(aq) + K2SO4(aq), the complete ionic equation is Fe2+(aq) + SO42-(aq) + 2K+(aq) + 2Cl-(aq) -> Fe2+(aq) + 2Cl-(aq) + 2K+(aq) + SO42-(aq), and the net ionic equation is SO42-(aq) + 2K+(aq) -> 2K+(aq) + SO42-(aq).

Now, let's sprinkle some humor into it:

The equation is like a party where FeSO4 decides to mingle with KCl. They mix, dance, and it's electrifying! But when everyone sobered up, Fe2+ realized it didn't really want to hang out with K+ anymore, so it makes an excuse and leaves with 2Cl-. What's left is K2SO4, two K+ ions hooking up, and SO4-- sulking in the corner, wondering where Fe2+ went. And that's the story of FeSO4(aq) + KCl(aq) equation, where Fe2+ was a bit of a party pooper!

To write the balanced formula equation, the complete ionic equation, and the net ionic equation for the reaction between FeSO4(aq) and KCl(aq), we need to follow these steps:

Step 1: Write the balanced formula equation by combining the reactants and products.

The balanced formula equation is: FeSO4(aq) + 2KCl(aq) → FeCl2(aq) + K2SO4(aq)

Step 2: Write the complete ionic equation by separating the soluble ionic compounds into their respective ions.

The complete ionic equation is: Fe2+(aq) + SO4^2-(aq) + 2K+(aq) + 2Cl^-(aq) → FeCl2(aq) + K2SO4(aq)

Step 3: Write the net ionic equation by removing the spectator ions, which are present on both sides of the equation.

The net ionic equation is: Fe2+(aq) + 2Cl^-(aq) → FeCl2(aq)

To determine the balanced formula equation, complete ionic equation, and net ionic equation for the reaction between FeSO4 (aq) and KCl (aq), we need to first write the chemical equations and then break them down.

The balanced formula equation represents the overall reaction in terms of formulas and includes both reactants and products. It is obtained by combining the formulas of the reactants and products while ensuring that the number of each type of atom is the same on both sides of the equation.

The balanced formula equation for the reaction between FeSO4 (aq) and KCl (aq) is:

FeSO4(aq) + 2KCl(aq) → FeCl2(aq) + K2SO4(aq)

To obtain the complete ionic equation, we need to break down all the reactants and products into their respective ions. In ionic equations, soluble ionic compounds are split into their constituent ions.

FeSO4(aq) breaks down into:
Fe2+(aq) + SO4^2-(aq)

KCl(aq) breaks down into:
2K+(aq) + 2Cl-(aq)

FeCl2(aq) breaks down into:
Fe2+(aq) + 2Cl-(aq)

K2SO4(aq) breaks down into:
2K+(aq) + SO4^2-(aq)

Based on the above breakdown, the complete ionic equation is:

Fe2+(aq) + SO4^2-(aq) + 2K+(aq) + 2Cl-(aq) → Fe2+(aq) + 2Cl-(aq) + 2K+(aq) + SO4^2-(aq)

To obtain the net ionic equation, we remove the spectator ions, which are the ions that appear on both sides of the equation and do not participate in the reaction. In this case, the Fe2+ and K+ ions are spectator ions.

Removing the spectator ions from the complete ionic equation, we get the net ionic equation:

SO4^2-(aq) + 2Cl-(aq) → 2Cl-(aq) + SO4^2-(aq)

The net ionic equation simplifies to:

2Cl-(aq) → 2Cl-(aq)

Therefore, the net ionic equation does not involve any chemical changes and indicates that no reaction occurs.