The percentage yield for the reaction
PCL3+Cl2-->PCL5 is 83.2%. What mass of PCL5 is expected from the reaction of 73.7g of PCL3 with excess chlorine?
76.7g PCl3 x 0.832 = ?g PCl5
To find the mass of PCl5 expected from the reaction, we first need to calculate the theoretical yield. The theoretical yield represents the maximum amount of product that can be formed under ideal conditions.
1. Start by determining the balanced chemical equation for the reaction:
PCl3 + Cl2 → PCl5
2. Calculate the molar masses of the compounds involved:
- PCl3: 31.0 g/mol (1 phosphorus atom + 3 chlorine atoms)
- Cl2: 70.9 g/mol (2 chlorine atoms)
- PCl5: 208.2 g/mol (1 phosphorus atom + 5 chlorine atoms)
3. Convert the mass of PCl3 to moles:
mass of PCl3 = 73.7 g
moles of PCl3 = mass of PCl3 / molar mass of PCl3 = 73.7 g / 137.3 g/mol = 0.5362 mol
4. Use the stoichiometry of the balanced equation to determine the mole ratio between PCl3 and PCl5. In this case, the mole ratio is 1:1, meaning 1 mole of PCl3 reacts to produce 1 mole of PCl5.
5. Since we have a 100% excess of Cl2, we assume that all the PCl3 has reacted, and the limiting reagent is PCl3. Therefore, the number of moles of PCl5 formed is also 0.5362 mol.
6. Calculate the theoretical yield of PCl5 in grams:
mass of PCl5 = moles of PCl5 × molar mass of PCl5 = 0.5362 mol × 208.2 g/mol = 111.6 g
So, the theoretical yield of PCl5 from the reaction is 111.6 grams.
To find the expected mass of PCl5 based on the given percentage yield, we can multiply the theoretical yield by the percentage yield:
expected mass of PCl5 = theoretical yield × percentage yield
expected mass of PCl5 = 111.6 g × 0.832
Therefore, the expected mass of PCl5 from the reaction of 73.7g of PCl3 with excess chlorine is approximately 92.74 grams.
To determine the mass of PCl₅ expected from the reaction, we need to use the concept of percentage yield. The percentage yield is the ratio of the actual yield to the theoretical yield, multiplied by 100.
In this case, the percentage yield is given as 83.2%, which means that 83.2% of the theoretical yield is obtained. Therefore, we can calculate the theoretical yield as follows:
Step 1: Calculate the molar mass of PCl₃ and PCl₅
- PCl₃: P (1 atom) + Cl (3 atoms) = 31 g/mol + (3 x 35.5 g/mol) = 137.5 g/mol
- PCl₅: P (1 atom) + Cl (5 atoms) = 31 g/mol + (5 x 35.5 g/mol) = 208.5 g/mol
Step 2: Calculate the moles of PCl₃
- Moles = Mass / Molar Mass
- Moles = 73.7 g / 137.5 g/mol = 0.536 mol
Step 3: Use stoichiometry to determine the moles of PCl₅ produced
- From the balanced equation, we can see that the molar ratio of PCl₃ to PCl₅ is 1:1
- Therefore, the moles of PCl₅ produced would also be 0.536 mol
Step 4: Calculate the mass of PCl₅ expected
- Mass = Moles x Molar Mass
- Mass = 0.536 mol x 208.5 g/mol = 111.8 g
Therefore, the expected mass of PCl₅ from the reaction of 73.7 g of PCl₃ with excess chlorine is 111.8 g.