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Solved: For the reaction shown, calculate the theoretical yield of the product in grains
Chapter 8, Problem 58P(choose chapter or problem)
For the reaction shown, calculate the theoretical yield of the product in grams for each of the initial quantities of reactants.
\(\mathrm{Ti}(s)+2 \mathrm{~F}_{2}(\mathrm{~g}) \rightarrow \mathrm{TiF}_{4}(s)\)
\(\begin{array}{l}\text{(a) }1.0\mathrm{\ g}\mathrm{\ Ti};\ 1.0\mathrm{\ g}\mathrm{F}_2\\ \text{(b) }4.8\mathrm{\ g}\mathrm{\ Ti};\ 3.2\mathrm{\ g}\mathrm{\ F}_2\\ \text{(c) }0.388\mathrm{\ g\ }\mathrm{Ti};\ 0.341\mathrm{\ g}\mathrm{\ F}_2\end{array}\)
Questions & Answers
QUESTION:
For the reaction shown, calculate the theoretical yield of the product in grams for each of the initial quantities of reactants.
\(\mathrm{Ti}(s)+2 \mathrm{~F}_{2}(\mathrm{~g}) \rightarrow \mathrm{TiF}_{4}(s)\)
\(\begin{array}{l}\text{(a) }1.0\mathrm{\ g}\mathrm{\ Ti};\ 1.0\mathrm{\ g}\mathrm{F}_2\\ \text{(b) }4.8\mathrm{\ g}\mathrm{\ Ti};\ 3.2\mathrm{\ g}\mathrm{\ F}_2\\ \text{(c) }0.388\mathrm{\ g\ }\mathrm{Ti};\ 0.341\mathrm{\ g}\mathrm{\ F}_2\end{array}\)
ANSWER:
Step 1 of 4
The given equation.
\(\mathrm{Ti}(\mathrm{s})+2 \mathrm{~F}_{2}(\mathrm{~g}) \rightarrow \mathrm{TiF}_{4}(\mathrm{~s})\)
Limiting reactant is the reactant that is completely consumed in a chemical reaction.
Theoretical yield-the amount of product that can be made in a chemical reaction based on the amount of limiting reactant.