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The percentage yield for the reaction
PCl3 + Cl2 → PCl5
is 83.2%. What mass of PCl5 is expected from the reaction of 73.7 g PCl3 with excess chlorine?

Respuesta :

superman1987

Answer:

92.87 g.

Explanation:

∵ The percentage yield = (actual yield/theoretical yield)*100.

  • We need to calculate the theoretical yield:

From the balanced reaction:

PCl₃ + Cl₂ → PCl₅,

It is clear that 1 mol of PCl₃ reacts with 1 mol of Cl₂ to produce 1 mol of PCl₅.

  • We need to calculate the no. of moles of 73.7 g PCl₃:

n = mass/molar mass = (73.7 g)/(137.33 g/mol) = 0.536 mol.

Using cross multiplication:

1 mol of PCl₃ produce  → 1 mol of PCl₅, from stichiometry.

∴ 0.536 mol of PCl₃ produce  → 0.536 mol of PCl₅.

∴ The mass of PCl₅ (theoretical yield) = (no. of moles) * (molar mass) = (0.536 mol)*(208.24 g/mol) = 111.62 g.

∵ The percentage yield = (actual yield/theoretical yield)*100.

The percentage yield = 83.2%, theoretical yield = 111.62 g.

∴ The actual yield of PCl₅ = (The percentage yield)(theoretical yield)/100 = (83.2%)(111.62 g)/100 = 92.87 g.

CintiaSalazar

Considering the definition of percent yield, if the percentage yield for the reaction  is 83.2%, 92.97 grams of PCl₅ is expected from the reaction of 73.7 g PCl₃ with excess chlorine.

The balanced reaction is:

PCl₃ + Cl₂ → PCl₅

Theorical yield

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

  • PCl₃: 1 mole
  • Cl₂: 1 mole
  • PCl₅: 1 mole

The molar mass of the compounds is:

  • PCl₃: 137.35 g/mole
  • Cl₂: 70.9 g/mole
  • PCl₅: 208.25 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

  • PCl₃: 1 mole× 137.35 g/mole= 137.35 grams
  • Cl₂: 1 mole× 70.9 g/mole= 70.9 grams
  • PCl₅: 1 mole× 208.25 g/mole= 208.25 grams

Then the following rule of three can be applied: if by reaction stoichiometry 137.35 grams of PCl₃ form 208.25 grams of PCl₅, 73.7 grams of PCl₃ form how much mass of PCl₅?

[tex]amount of mass of PCl_{5} =\frac{73.7 grams of PCl_{3} x208.25 grams of PCl_{5}}{137.35 grams of PCl_{3}}[/tex]

amount of mass of PCl₅= 111.74 grams

Definition of percent yield

The percent yield is defined as the ratio of the actual return to the theoretical return expressed as a percentage.

The percent yield is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:

[tex]percent yield=\frac{actual yield}{theorical yield} x100[/tex]

where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.

Calculation of actual yield

In this case, you know:

percent yield= 83.2%

actual yield= ?

theorical yield= 111.74 grams

Replacing in the definition of percent yields:

[tex]83.2=\frac{actual yield}{111.74 grams} x100[/tex]

Solving:

[tex]actual yield=\frac{83.2x111.74 grams}{100}[/tex]

actual yield=92.97 grams

If the percentage yield for the reaction  is 83.2%, 92.97 grams of PCl₅ is expected from the reaction of 73.7 g PCl₃ with excess chlorine.

Learn more about percent yield:

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