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loulou6166
09.03.2020 •
Chemistry
Using the above equation, how many moles of sulfur can be produced if 0.5640 moles of sulfur dioxide are used with excess hydrogen sulfide?
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Ответ:
Explanation:
1. Write the balanced chemical equation
2H₂S + SO₂ → 2H₂O + 3S
2. State the mole ratio
3. Calculate the moles of S
Moles S = 0.5640 mol SO₂ × (3 mol S / 1 mol SO₂) = 1.692 mol SОтвет:
The actual yield is 125.65 g.
Explanation:
The balanced equation is: 2 Na + Cl₂ → 2 NaCl.From the stichiometry of this balanced equation: 2.0 moles of Na reacts with 1.0 mole of chlorine gas to give 2.0 moles of NaCl.We need to calculate the number of moles of Na (n = mass/atomic mass), n = (57.50 g / 22.989 g/mole of Na) = 2.5 mole.Using cross multiplication and from stichiometry:
2.0 moles of Na → 2.0 moles of NaCl
2.5 moles of Na → 2.5 moles of NaCl
Now, we can calculate the mass of the produced NaCl (m = n x molar mass)m = (2,5 mole x 58.443 g/mole of NaCl) = 146.1 g.This is the yield if the percentage of yield is 100%, but the percentage yield of the reaction is 86%.The actual yield = (146.1 g) (86/100) = 125.65 g.