Hi I think I might know the answer to your question it is pretty tricky though!
Chlorine Gas = 70.8 grams/moles
Moles of Chlorine Gas = 57.8/70.8 = 0.816 mol
Volume Gas at STP = 22.4 L/mol
Volume of Chlorine Gas = .816*22.4=18.22 Litters
I hoped that helps if not so sorry!
Answer: the percent yield of NaCl in the experiement is 109%.
Explanation:
1) <u><em>Each mole of HCl consumed should produce a mole of NaCl product</em></u>
⇒ 1 mol HCl / 1 mol NaCl
2) <u>Reactant</u><em><u>: 10.9 grams of HCl (36.5 g/mol) </u></em>
- Convert grams to moles: moles = mass in grams / molar mass
- moles = 10.9 g / 36.5 g/mol = 0.299 mol HCl
3) <u>Theoretical (stoichiometric) yield of NaCl</u>
- Set the proportion: 1 mol HCl / 1 mol NaCl = 0.299 mol HCl / x
⇒ x = 0.299 mol NaCl (should be obtained)
4) <u>Actual yield</u>
- 19 grams of NaCl (58.5 g/mol)
- Convert to moles: moles = mass in grams / molar mass
- moles = 19 g / 58.5 g/mol = 0.325 mol NaCl
5) <em><u>Percent yield</u></em>:
- Equation: percent yield = (actual yiel / theoretical yield) × 100
- Percent yiedl = 109% ← answer
<u>Note:</u> it is not normal to obtain percent yields greater than 100%. When this happens, you must think in an experimental error or that the sample was contaminated with some substance that yield to an increase of the measured product.