Question

Given the balanced reaction equation 16s2f2 → 3s8 + 8sf4, what is the percent yield for the reaction if the reaction of 78.76 g of s2f2 yields 33.48 g of sf4?

Answer 1

The percent yield of SF4 is calculated using the actual yield (33.48 g) and the theoretical yield determined by stoichiometry. The theoretical yield is calculated from the balanced equation and the mass of S2F2 that reacted (78.76 g); then, apply the formula for percent yield.

Step-by-step explanation:

To calculate the percent yield of SF4 we first need to determine the theoretical yield using stoichiometry from the balanced reaction equation 16S2F2 → 3S8 + 8SF4. Since 16 moles of S2F2 produce 8 moles of SF4, we can set up a ratio to find the moles of SF4 that should have been produced from the actual amount of S2F2 reacted (78.76 g).

We do this in several steps:

1. Convert the mass of S2F2 to moles.
2. Use the mole ratio from the equation to find the moles of SF4 expected.
3. Convert moles of SF4 to grams to find the theoretical yield.

From there, percent yield is calculated using the formula:

Percent Yield = (Actual Yield / Theoretical Yield) × 100%

The actual yield is given as 33.48 g of SF4. After completing all stoichiometric calculations, you would then divide 33.48 g (actual yield) by the theoretical yield in grams and multiply by 100 to obtain the percent yield.