Question

Sulfur and oxygen react to produce sulfur trioxide. In a particular experiment, 7.9 grams of SO3 are produced by the reaction of 5.0 grams of O2 with 6.0 grams of S. What is the % yield of SO3 in this experiment?

Answer 1

To calculate the percent yield of SO3 in this experiment, we need to compare the actual yield of SO3 to the theoretical yield. The theoretical yield can be calculated using stoichiometry. Once we have the theoretical yield, we can calculate the percent yield using the formula (Actual Yield / Theoretical Yield) x 100%.

Step-by-step explanation:

To calculate the percent yield of SO3 in this experiment, we need to compare the actual yield of SO3 to the theoretical yield. The theoretical yield can be calculated using stoichiometry. First, we need to determine the limiting reactant. From the given masses, we can calculate the moles of O2 and S. Then, we compare the mole ratios between O2 and S in the balanced chemical equation to determine which reactant is limiting. Once we have the limiting reactant, we can calculate the theoretical yield of SO3 using the mole ratio with respect to the limiting reactant.

Once we have the theoretical yield, we can calculate the percent yield using the formula:

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

Substituting the given values, we get:

Percent Yield = (7.9 g / Theoretical Yield) x 100%