Questions: The following chemical reaction takes place in aqueous solution: FeBr2(aq) + Na2S(aq) → FeS(s) + 2 NaBr(aq) Write the net ionic equation for this reaction.

The following chemical reaction takes place in aqueous solution:
FeBr2(aq) + Na2S(aq) → FeS(s) + 2 NaBr(aq)

Write the net ionic equation for this reaction.

Transcript text: The following chemical reaction takes place in aqueous solution: \[ \mathrm{FeBr}_{2}(a q)+\mathrm{Na}_{2} \mathrm{~S}(a q) \rightarrow \mathrm{FeS}(s)+2 \mathrm{NaBr}(a q) \] Write the net ionic equation for this reaction.

Solution

Solution Steps

Step 1: Write the Balanced Molecular Equation

The given balanced molecular equation is: \[ \mathrm{FeBr}_{2}(aq) + \mathrm{Na}_{2}\mathrm{S}(aq) \rightarrow \mathrm{FeS}(s) + 2\mathrm{NaBr}(aq) \]

Step 2: Write the Complete Ionic Equation

In aqueous solutions, soluble ionic compounds dissociate into their respective ions. Therefore, the complete ionic equation is: \[ \mathrm{Fe}^{2+}(aq) + 2\mathrm{Br}^-(aq) + 2\mathrm{Na}^+(aq) + \mathrm{S}^{2-}(aq) \rightarrow \mathrm{FeS}(s) + 2\mathrm{Na}^+(aq) + 2\mathrm{Br}^-(aq) \]

Step 3: Identify and Remove Spectator Ions

Spectator ions are ions that appear on both sides of the equation and do not participate in the reaction. In this case, the spectator ions are \(\mathrm{Na}^+\) and \(\mathrm{Br}^-\).

Step 4: Write the Net Ionic Equation

After removing the spectator ions, the net ionic equation is: \[ \mathrm{Fe}^{2+}(aq) + \mathrm{S}^{2-}(aq) \rightarrow \mathrm{FeS}(s) \]