1. Determine the limiting reactant:
* Convert grams to moles:
* Moles of K = (1.446 g K) / (39.10 g/mol K) = 0.0370 mol K
* Moles of Cl = (8.178 g Cl) / (35.45 g/mol Cl) = 0.230 mol Cl
* Determine the mole ratio from the balanced chemical equation:
2K + Cl₂ → 2KCl
The ratio is 2 moles of K react with 1 mole of Cl₂.
* Calculate the moles of Cl₂ needed to react with all of the K:
(0.0370 mol K) * (1 mol Cl₂ / 2 mol K) = 0.0185 mol Cl₂
* Compare the moles of Cl₂ needed to the moles of Cl₂ available:
0.0185 mol Cl₂ (needed) < 0.230 mol Cl₂ (available)
Conclusion: Potassium is the limiting reactant because there's not enough of it to react with all of the chlorine.
2. Calculate the mass of KCl produced:
* Use the mole ratio from the balanced equation:
(0.0370 mol K) * (2 mol KCl / 2 mol K) = 0.0370 mol KCl
* Convert moles of KCl to grams:
(0.0370 mol KCl) * (74.55 g/mol KCl) = 2.76 g KCl
Answer:
The 1.446 g sample of potassium will react completely with a portion of the 8.178 g of chlorine, producing 2.76 g of potassium chloride (KCl). There will be excess chlorine remaining.
