Stoichiometry Trivia Test: MCQ Quiz!

Reviewed by Editorial Team
The ProProfs editorial team is comprised of experienced subject matter experts. They've collectively created over 10,000 quizzes and lessons, serving over 100 million users. Our team includes in-house content moderators and subject matter experts, as well as a global network of rigorously trained contributors. All adhere to our comprehensive editorial guidelines, ensuring the delivery of high-quality content.
Learn about Our Editorial Process
| By Tbautista
T
Tbautista
Community Contributor
Quizzes Created: 1 | Total Attempts: 563
| Attempts: 565
Quiz Flashcard
SettingsSettings
Please wait...
  • 1/9 Questions
    Ammonia, , and copper (II) oxide react to form solid copper, water and nitrogen gas. What are the coefficients for the balanced chemical equations. - ProProfs

    Ammonia, , and copper (II) oxide react to form solid copper, water and nitrogen gas. What are the coefficients for the balanced chemical equations.

    • 2,2,2,1,1
    • 1,2,1,2,1
    • 2,3,3,3,1
Please wait...
About This Quiz

Stoichiometry Trivia Test: MCQ Quiz! Explore the fundamentals of chemical reactions through questions on reaction coefficients, limiting and excess reactants, and the calculation of product masses. This quiz assesses your ability to apply stoichiometric principles in practical scenarios, enhancing your understanding of chemistry.

Stoichiometry Trivia Test: MCQ Quiz! - Quiz

Quiz Preview

  • 2. 

    If 40g of ammonia reacts with 80.0g copper (II) oxide, determine the limiting reactant. Use nitrogen gas as your unknown.

    • Ammonia

    • Copper(II) oxide

    Correct Answer
    A. Copper(II) oxide
    Explanation
    In order to determine the limiting reactant, we need to compare the amount of ammonia and copper (II) oxide used in the reaction. The molar mass of ammonia (NH3) is 17.03 g/mol, so 40g of ammonia is approximately 2.35 moles. The molar mass of copper (II) oxide (CuO) is 79.55 g/mol, so 80.0g of copper (II) oxide is approximately 1.00 mole. Since the molar ratio between ammonia and copper (II) oxide is 2:1, we can see that there are more moles of ammonia than copper (II) oxide. Therefore, copper (II) oxide is the limiting reactant in this reaction.

    Rate this question:

  • 3. 

    Determine the mass of nitrogen gas produced in the reaction.

    • 9.4 g

    • 14.0g

    • 28.0 g

    Correct Answer
    A. 9.4 g
    Explanation
    The mass of nitrogen gas produced in the reaction is 9.4 g.

    Rate this question:

  • 4. 

    Which reactant is the excess reactant?

    • Ammonia

    • Copper(II) oxide

    Correct Answer
    A. Ammonia
    Explanation
    In a chemical reaction, the excess reactant is the reactant that is present in a greater amount than required for the reaction to proceed to completion. In this case, ammonia is the excess reactant because it is mentioned first in the list of reactants. This implies that there is an excess amount of ammonia compared to copper(II) oxide, indicating that ammonia is present in a greater quantity than necessary for the reaction.

    Rate this question:

  • 5. 

    How much of the excess reactant remains after the reaction? **Ammonia is the excess reactant, meaning it will not be completely used up in a reaction. In other words, you will not be using all 40g of ammonia given. In order to find out how much is left over after the reaction, do a mass-mass problem. 80g CuO is the given and grams of ammonia is the unknown. This answer is how much ammonia is used up. Now, figure out how much is leftover!

    • 19.8 g

    • 32.4 g

    • 28.6 g

    Correct Answer
    A. 28.6 g
    Explanation
    Ammonia is the excess reactant, meaning it will not be completely used up in the reaction. To determine how much is left over, a mass-mass problem can be used. The given mass of copper(II) oxide (CuO) is 80g, and the mass of ammonia is the unknown. The answer, 28.6g, represents the amount of ammonia that is used up in the reaction, while the remaining amount is the excess reactant that remains.

    Rate this question:

  • 6. 

    When copper(II) oxide is heated with hydrogen gas, water and copper metal is produced. What mass of copper can be obtained if 32.0g of copper(II) oxide is used?

    • 24.3g

    • 25.5g

    • 27.6g

    Correct Answer
    A. 25.5g
    Explanation
    When copper(II) oxide is heated with hydrogen gas, a chemical reaction occurs and water and copper metal are produced. The balanced chemical equation for this reaction is: CuO + H2 → Cu + H2O. According to the equation, 1 mole of copper(II) oxide (CuO) reacts to produce 1 mole of copper (Cu). To find the mass of copper that can be obtained, we need to convert the mass of copper(II) oxide (32.0g) to moles using its molar mass (79.55g/mol), and then use the mole ratio from the balanced equation to find the mass of copper produced. The calculation gives us a mass of approximately 25.5g of copper.

    Rate this question:

  • 7. 

    Nitrogen monoxide reacts with oxygen gas to produce nitrogen dioxide. What are the coefficients that balance the equation?

    • 2,1,2

    • 1,2,1

    • 2,1,1

    Correct Answer
    A. 2,1,2
    Explanation
    The coefficients that balance the equation are 2, 1, 2. This means that 2 molecules of nitrogen monoxide react with 1 molecule of oxygen gas to produce 2 molecules of nitrogen dioxide. The balanced equation is 2NO + O2 -> 2NO2.

    Rate this question:

  • 8. 

    What is the theoretical yield of hydrogen gas if 36.0 g of water decomposes to produce hydrogen gas and oxygen gas?

    • 2.02 g H2

    • 1.01 g H2

    • 4.04 g H2

    Correct Answer
    A. 4.04 g H2
    Explanation
    The theoretical yield of hydrogen gas can be calculated using the stoichiometry of the reaction. The balanced equation for the decomposition of water is 2H2O -> 2H2 + O2. From the equation, we can see that for every 2 moles of water, we get 2 moles of hydrogen gas. The molar mass of water is 18.02 g/mol, so 36.0 g of water is equal to 2 moles. Therefore, the theoretical yield of hydrogen gas is also 2 moles, which is equal to 4.04 g H2.

    Rate this question:

  • 9. 

    What is the percent yield of hydrogen gas if 3.80g of hydrogen is collected in the lab?

    • 94%

    • 88%

    • 96%

    Correct Answer
    A. 94%

Quiz Review Timeline (Updated): Mar 21, 2023 +

Our quizzes are rigorously reviewed, monitored and continuously updated by our expert board to maintain accuracy, relevance, and timeliness.

  • Current Version
  • Mar 21, 2023
    Quiz Edited by
    ProProfs Editorial Team
  • Nov 27, 2013
    Quiz Created by
    Tbautista

Related Topics

Recent Quizzes

Stoichiometry Trivia Test: MCQ Quiz! Stoichiometry Trivia Test: MCQ Quiz!
Aqueous Reactions and Solution Stoichiometry Test Prep. Aqueous Reactions and Solution Stoichiometry Test Prep.
topic 7: stoichiometry part 1 topic 7: stoichiometry part 1

Featured Quizzes

Harry Potter House Quiz: Which Hogwarts House Do You Belong To? Harry Potter House Quiz: Which Hogwarts House Do You Belong To?
Introduction to Computer: MCQ Questions With Answers Introduction to Computer: MCQ Questions With Answers
Are You Ready For IQ Quiz: Test Your Intelligence Now Are You Ready For IQ Quiz: Test Your Intelligence Now
Can You Guess These Asian's Nationality? Can You Guess These Asian's Nationality?
What Ethnicity Do I Look Like? What Ethnicity Do I Look Like?
Basketball Quiz Questions And Answers Basketball Quiz Questions And Answers
Back to Top Back to top
Advertisement
×

Wait!
Here's an interesting quiz for you.

We have other quizzes matching your interest.