30.0g of tin metal and 15.0g of hydrogen fluoride react to produce tin(II) fluoride and hydrogen gas.
1. Write the balanced formula equation
2. What is the limiting reactant
3. How many grams of hydrogen gas can be produced?
4. How much excess reactant will you have left?
Answers
Explanation:
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Contents Home Campus Bookshelves Oregon Institute of Technology OIT: CHE 201 - General Chemistry I Unit 5: Transformations of Matter Expand/collapse global location
5.3: Calculating Reaction Yields (Problems)
Last updatedSep 19, 2020
5.3: Calculating Reaction Yields
Unit 6: Common Chemical Reactions
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PROBLEM 5.3.1
The following quantities are placed in a container: 1.5 × 1024 molecules of diatomic hydrogen, 1.0 mol of sulfur, and 88.0 g of diatomic oxygen.
What is the total mass in grams for the collection of all three elements?
What is the total number of moles of atoms for the three elements?
If the mixture of the three elements formed a compound with molecules that contain two hydrogen atoms, one sulfur atom, and four oxygen atoms, which substance is consumed first?
How many atoms or molecules of each remaining element would remain unreacted in the change described above ?
Answer a
Answer b
Answer c
Answer d
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PROBLEM 5.3.2
What is the limiting reactant in a reaction that produces sodium chloride from 8 g of sodium and 8 g of diatomic chlorine?
Answer
PROBLEM 5.3.3
Which of the postulates of Dalton's atomic theory explains why we can calculate a theoretical yield for a chemical reaction?
Answer
PROBLEM 5.3.4
A student isolated 25 g of a compound following a procedure that would theoretically yield 81 g. What was his percent yield?
Answer
PROBLEM 5.3.5
A sample of 0.53 g of carbon dioxide was obtained by heating 1.31 g of calcium carbonate. What is the percent yield for this reaction?
CaCO3(s)→CaO(s)+CO2(s)(5.3.1)
Answer
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PROBLEM 5.3.6
Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of CCl4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.
Answer
PROBLEM 5.3.7
Citric acid, C6H8O7, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger. The equation representing this reaction is
C12H22O11+H2O+3O2→2C6H8O7+4H2O(5.3.2)