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Chemical Combo: How N2 and F2 Produce Nitrogen Trifluoride Explained!
Chapter 6, Problem 6.43(choose chapter or problem)
The balanced equation for the reaction of nitrogen and fluorine to form nitrogen trifluoride is
\(\mathrm{N}_2(g)+3\mathrm{F}_2(g)\longrightarrow2\mathrm{NF}_3(g)\)
Assume that 10.0 g of \(\rm{N}_2\) is mixed with 10.0 g of \(\rm{F}_2\).
(a) What is the limiting reactant?
(b) What is the maximum amount of \(\mathrm{NF}_3\), in grams, that can be produced?
Questions & Answers
QUESTION:
The balanced equation for the reaction of nitrogen and fluorine to form nitrogen trifluoride is
\(\mathrm{N}_2(g)+3\mathrm{F}_2(g)\longrightarrow2\mathrm{NF}_3(g)\)
Assume that 10.0 g of \(\rm{N}_2\) is mixed with 10.0 g of \(\rm{F}_2\).
(a) What is the limiting reactant?
(b) What is the maximum amount of \(\mathrm{NF}_3\), in grams, that can be produced?
ANSWER:Step 1 of 3
Limiting reagent and theoretical yield
Determining limiting reagent and theoretical yield involves using stoichiometry obtained from the balanced chemical equation.
Limiting reagent: The reagent whose concentration is less than the required relative amount obtained from the stoichiometric calculation is the limiting reagent. As it has a lower relative concentration, it reacts completely in the reaction to form the product.
Theoretical yield: The maximum amount of product generated from a given amount of reactants. The limiting reagent governs theoretical yield as this reagent is completely converted into the product in an idealized reaction.
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Chemical Combo: How N2 and F2 Produce Nitrogen Trifluoride Explained!
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Explore the chemical combination of nitrogen and fluorine to produce nitrogen trifluoride. Learn how to determine the limiting reactant and calculate the theoretical yield using stoichiometry principles.