Sure, let's solve this step-by-step.
We are given the balanced chemical reaction:
[tex]\[ \text{FeCl}_2 + 2 \text{NaOH} \rightarrow \text{Fe(OH)}_2(s) + 2 \text{NaCl} \][/tex]
We need to determine how many moles of NaOH will be used up if 6 moles of FeCl₂ are added to 6 moles of NaOH.
1. Identify the stoichiometric ratios from the balanced equation:
- According to the balanced equation, 1 mole of FeCl₂ reacts with 2 moles of NaOH.
2. Determine the moles of NaOH needed for the given moles of FeCl₂:
- To react with 6 moles of FeCl₂, based on the 1:2 ratio, we need:
[tex]\[
6 \text{ moles of FeCl}_2 \times 2 \frac{\text{moles of NaOH}}{\text{mole of FeCl}_2} = 12 \text{ moles of NaOH}
\][/tex]
3. Compare the required moles of NaOH with the moles available:
- We need 12 moles of NaOH to completely react with 6 moles of FeCl₂.
- However, we only have 6 moles of NaOH available.
4. Determine the limiting reagent:
- Since NaOH is less than the amount required, NaOH is the limiting reagent in this reaction.
5. Calculate the moles of NaOH that will be used up:
- Since NaOH is the limiting reagent, all 6 moles of NaOH will be used up in the reaction.
So, the number of moles of NaOH that will be used up is:
[tex]\[
\boxed{6}
\][/tex]
