Write the net ionic equation (including phases) that corresponds to Fe(ClO4)2(aq)+Na2S(aq)=FeS(s)+2NaClO4(aq)
To write the net ionic equation, we need to first write the balanced equation for the given reaction.
The balanced equation for the reaction Fe(ClO4)2(aq) + Na2S(aq) = FeS(s) + 2NaClO4(aq) is:
2Fe(ClO4)2(aq) + 3Na2S(aq) = FeS(s) + 4NaClO4(aq)
Now, let's break down the equation into its respective ionic species and write the net ionic equation.
First, determine which species remain unchanged in both the reactants and products. These species are called spectator ions and will be omitted from the net ionic equation.
The spectator ions in this reaction are 2Na+(aq) and 2ClO4-(aq).
Now, let's write the net ionic equation by removing the spectator ions:
Fe(ClO4)2(aq) + 3Na2S(aq) = FeS(s) + 4NaClO4(aq)
Net Ionic Equation: 2Fe2+(aq) + 3S2-(aq) = FeS(s)
To write the net ionic equation for the reaction Fe(ClO4)2(aq) + Na2S(aq) = FeS(s) + 2NaClO4(aq), we need to first write the balanced molecular equation and then convert it to the net ionic equation by canceling out the spectator ions.
Step 1: Write the balanced molecular equation.
Fe(ClO4)2(aq) + Na2S(aq) → FeS(s) + 2NaClO4(aq)
Step 2: Split all the soluble ionic compounds into their respective ions.
Fe(ClO4)2(aq) → Fe^2+(aq) + 2ClO4^-(aq)
Na2S(aq) → 2Na+(aq) + S^2-(aq)
FeS(s) → Fe^2+(aq) + S^2-(aq)
2NaClO4(aq) → 2Na+(aq) + 2ClO4^-(aq)
Step 3: Write the net ionic equation by canceling out spectator ions (ions that appear on both sides of the equation and do not participate in the reaction).
We can see that Fe^2+ and S^2- ions appear on both sides of the equation, so they cancel out.
Net ionic equation: Fe^2+(aq) + S^2-(aq) → FeS(s)
Therefore, the net ionic equation for the reaction Fe(ClO4)2(aq) + Na2S(aq) = FeS(s) + 2NaClO4(aq) is Fe^2+(aq) + S^2-(aq) → FeS(s).
You have the molecular equation.
Step 1. Convert to the ionic equation with these rules.
a. ppts are written as molecules.
b. gases are as molecules.
c. weak electrolytes (weak acids, weak bases, water, etc) are written as molecules.
d. everything else is written as ions (example: all of the aqueous solution are written as ions.
Step 2. Look at both sides of the equation and cancel ions that appear on both sides. What is left is the net ionic equation.