Percent Yield Lesson
Presentation
•
Chemistry
•
9th - 12th Grade
•
Medium
Standards-aligned
Shane Pulliam
Used 5+ times
FREE Resource
17 Slides • 6 Questions
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Drag and Drop
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Multiple Choice
Four students were tasked with running an experiment in which they needed to produce hydrogen gas from the following reaction. Which student had the worst efficiency?
Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)
Student 1 had an 84.2% yield.
Student 2 had an 89.1% yield.
Student 3 had an 89.7% yield.
Student 4 had an 86.5% yield.
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Math Response
The theoretical yield of ammonia produced when hydrogen and nitrogen react is 46.4 g. During a lab, only 39.1 g was produced. What is the percent yield of the ammonia?
Percent Yield: _____%
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First things first, you need to write a balanced chemical equation.
Balanced Chemical Equation
Write a word equation.
Write the chemical formulas for the reactants and the products.
Balance.
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Fill in the Blanks
What are the coefficients for the balanced chemical equation for the given problem?
A mass of 26.5 g of ammonia was produced when 7.00 g of hydrogen was reacted with excess nitrogen. What is the percent yield of ammonia produced?
Type answer...
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Fill in the Blanks
3 H2(g) + N2(g) → 2 NH3(g)
A mass of 26.5 g of ammonia was produced when 7.00 g of hydrogen was reacted with excess nitrogen. What is the theoretical yield?
Type answer...
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Math Response
3 H2(g) + N2(g) → 2 NH3(g)
A mass of 26.5 g of ammonia was produced when 7.00 g of hydrogen was reacted with excess nitrogen. What is the percent yield?
Percent Yield: ____ %
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