Top topic this week
Back to FAQs
Related FAQs
Frequently Asked Question
Questions asked by users might not always be phrased in the clearest way.
The percent yield for the reaction of phosphorus trichloride plus chlorine gas producing phosphorus pentachloride is 83.2%. What mass of PCl5 is expected form the reaction of 73.7g of phosphorus trichloride with excess chlorine?
Accepted Answer
Here's how to solve the problem:
1. Balanced Equation:
PCl3(l) + Cl2(g) → PCl5(s)
2. Calculate moles of PCl3:
Moles of PCl3 = mass / molar mass = 73.7 g / (30.97 g/mol + 3
35.45 g/mol) = 0.550 mol
3. Theoretical yield of PCl5:
The balanced equation shows a 1:1 mole ratio between PCl3 and PCl5. Therefore, the theoretical yield of PCl5 is also 0.550 mol.
4. Calculate mass of PCl5 (theoretical):
Mass of PCl5 = moles
molar mass = 0.550 mol
(30.97 g/mol + 5
35.45 g/mol) = 97.6 g
5. Calculate actual yield of PCl5:
Actual yield = percent yield
theoretical yield = 0.832
97.6 g = 81.2 g
Therefore, 81.2 g of PCl5 is expected to form from the reaction.
Articles you might like