1. Write and balance the equation.
2. Convert 8.7g F2 to mols. mols = grams/molar mass.
3. Using the coefficients in the balanced equation, convert mols F2 to mols of the product.
4. Convert mols product to grams. g = mols x molar mass. The is the theoretical yield (TE).\
5. %yield = (actual yield/TE)*100 = ?
3.9 g is the actual yield.
The reaction of 8.7 grams of fluorine with
excess chlorine produced 3.9 grams of ClF3.
What percent yield of ClF3 was obtained?
Answer in units of %
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