Ask Question
22 April, 03:17

A chemist reacted 17.25 grams of sodium metal with excess chlorine gas. The chemical reaction is as follows

Na + Cl2 → NaCl

If the percentage yield of the reaction is 88%, what is the actual yield?

+3
Answers (1)
  1. 22 April, 04:41
    0
    38.588 g ≅ 35.60 g.

    Explanation:

    From the balanced equation: 2Na + Cl₂ → 2NaCl, It is clear that 2.0 mole of Na reacts with 1.0 mole of Cl₂ to produce 2.0 mole NaCl. The no. of moles of Na metal reacted = mass / atomic mass = (17.25 g) / (22.989 g/mol) = 0.75 mol.

    Using cross multiplication:

    2.0 moles of Na metal produce → 2.0 moles of NaCl,

    ∴ 0.75 mole of Na metal produce → 0.75 mole of NaCl.

    The calculated (theoretical) yield of NaCl = n x molar mass = (0.75 mol) (58.44 g/mol) = 43.85 g.

    ∵ The percentage yield = [ (actual yield) / (calculated yield) ] x 100.

    ∴ The actual yield = [ (the percentage yield) (calculated yield) ] / 100 = [ (88 %) (43.85 g) ] / 100 = 38.588 g ≅ 35.60 g.
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “A chemist reacted 17.25 grams of sodium metal with excess chlorine gas. The chemical reaction is as follows Na + Cl2 → NaCl If the ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers