The reaction of 9.3 grams of fluorine with
excess chlorine produced 4.1 grams of ClF3.
What percent yield of ClF3 was obtained?
1. Write and balance the equation.
2. Convert 9.3 g F2 to mols. mols = grams/molar mass.
3. Using the coefficients in the balanced equation, convert mols F2 to mols of the product.l
4. Now convert mols or the product to grams. g = mols x molar mass. This is the theoretical yield(TE). Actual yield is 4.1g.
5. %yield = (actual yield/TE)*100 = ?
To calculate the percent yield of ClF3, we need to compare the actual yield to the theoretical yield. The theoretical yield is the maximum amount of product that can be obtained based on the balanced chemical equation.
Let's start by writing the balanced chemical equation for the reaction between fluorine (F2) and chlorine (Cl2) to produce chlorine trifluoride (ClF3):
F2 + 3Cl2 -> 2ClF3
According to the equation, we need 3 moles of Cl2 to react with 1 mole of F2 to produce 2 moles of ClF3. Let's calculate the moles of F2:
Molar mass of F2 = 19.0 g/mol
Moles of F2 = mass of F2 / molar mass of F2
= 9.3 g / 19.0 g/mol
≈ 0.489 mol
Since F2 and Cl2 react in a 1:3 ratio, the moles of Cl2 required can be calculated as follows:
Moles of Cl2 = 3 * moles of F2
= 3 * 0.489 mol
= 1.468 mol
Now, let's calculate the theoretical yield of ClF3 based on the moles of Cl2:
Molar mass of ClF3 = 83.45 g/mol (approximately)
Theoretical yield of ClF3 = moles of Cl2 * (molar mass of ClF3 / 3 moles of Cl2)
= 1.468 mol * (83.45 g/mol / 3)
≈ 40.59 g
Now, we can calculate the percent yield:
Percent yield = (actual yield / theoretical yield) * 100
= (4.1 g / 40.59 g) * 100
≈ 10.09 %
Therefore, the percent yield of ClF3 obtained is approximately 10.09%.
To determine the percent yield of ClF3, we need to compare the actual yield (4.1 grams) to the theoretical yield. The theoretical yield is the maximum amount of product that can be obtained based on stoichiometry.
First, let's calculate the theoretical yield of ClF3 using the balanced chemical equation for the reaction between fluorine (F2) and chlorine (Cl2) to produce ClF3.
1. Write the balanced chemical equation:
F2 + Cl2 -> 2ClF3
From the balanced equation, we can see that the molar ratio between F2 and ClF3 is 1:2. Therefore, to calculate the theoretical yield, we need to convert the mass of F2 to moles and then use the molar ratio to find the moles of ClF3, which can be converted to grams.
2. Calculate the moles of F2:
molar mass of F2 = 2 * atomic mass of F = 2 * 19 = 38 grams/mol
moles of F2 = mass of F2 / molar mass of F2 = 9.3 grams / 38 grams/mol
3. Calculate the moles of ClF3 using the molar ratio:
moles of ClF3 = moles of F2 * (2 moles of ClF3 / 1 mole of F2)
4. Calculate the theoretical yield of ClF3 in grams:
theoretical yield of ClF3 = moles of ClF3 * molar mass of ClF3
Now that we have the theoretical yield, we can calculate the percent yield.
5. Calculate the percent yield:
percent yield = (actual yield / theoretical yield) * 100
Using the given information, we have the actual yield as 4.1 grams.
Now you can follow the steps above to calculate the theoretical yield of ClF3 and then determine the percent yield.