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Consider the reaction between sulfur trioxide and
Chapter 8, Problem 62P(choose chapter or problem)
Consider the reaction between sulfur trioxide and water:
\(\mathrm{SO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(a q)\)
A chemist allows 61.5 g of \(\mathrm{SO}_{3}\) and 11.2 g of \(\mathrm{H}_{2} \mathrm{O}\) to react. When the reaction is finished, the chemist collects 54.9 g of \(\mathrm{H}_{2} \mathrm{SO}_{4}\). Determine the limiting reactant, theoretical yield, and percent yield for the reaction.
Questions & Answers
QUESTION:
Consider the reaction between sulfur trioxide and water:
\(\mathrm{SO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(a q)\)
A chemist allows 61.5 g of \(\mathrm{SO}_{3}\) and 11.2 g of \(\mathrm{H}_{2} \mathrm{O}\) to react. When the reaction is finished, the chemist collects 54.9 g of \(\mathrm{H}_{2} \mathrm{SO}_{4}\). Determine the limiting reactant, theoretical yield, and percent yield for the reaction.
ANSWER:
Step 1 of 5
Theoretical yield is the amount of product that can be made in a chemical reaction based on the amount of limiting reactant.
Actual yield is the amount of product actually produced by a chemical reaction.
\(\text { Percent yield }=\frac{\text { actual yield }}{\text { theoretical yield }} \times 100 \%\)