MCQs On Stoichiometry And Stoichiometric Calculations

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Janyce Wowk, BS (Chemistry) |
Chemistry
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Janyce is a chemistry professional with a B.S. in Chemistry from Montclair State University. Her experience as a research assistant and lab technician in a PFAS laboratory has allowed her to develop strong laboratory, data analysis, and research skills. On our review board team, Janyce reviews chemistry quizzes, ensuring accuracy and enhancing the quality of our educational materials. Her chemistry expertise and commitment to precision make her a valuable asset in maintaining high-quality resources for learners.
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MCQs On Stoichiometry And Stoichiometric Calculations - Quiz

Check out these MCQs on stoichiometry and stoichiometric calculations and see how good you're at using chemistry problems based on chemical formulas. Stoichiometry is a branch of chemistry that calculates various quantities of reactants and products of a chemical reaction using balanced chemical equations. How quickly can you solve a stoichiometric calculation accurately? Why don't you play the below quiz and see for yourself? Shall we begin the test? Best of luck, buddy!


Stoichiometry and Stoichiometric Calculations Questions and Answers

  • 1. 

    How many molecules are there in one mole of H2O?

    • A.

      6.023 x 1019

    • B.

      6.023 x 1023

    • C.

      1.084 x 1018

    • D.

      None of these

    Correct Answer
    B. 6.023 x 1023
    Explanation
    One mole of any substance contains Avogadro's number of particles, which is approximately 6.023 x 10^23. In the case of H2O, one mole of water contains 6.023 x 10^23 water molecules. Therefore, the correct answer is 6.023 x 10^23.

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  • 2. 

    A flask contains 500 cmof SOat STP. The flask contains?

    • A.

      40 g

    • B.

      100 g

    • C.

      50 g

    • D.

      1.427 g

    Correct Answer
    D. 1.427 g
    Explanation
    The given question states that a flask contains 500 cm3 of SO2 at STP. To determine the mass of the SO2 in the flask, we need to use the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. At STP, the pressure is 1 atm and the temperature is 273 K. We can rearrange the equation to solve for n, the number of moles. The molar mass of SO2 is 64 g/mol. By substituting the given values into the equation, we can calculate that n is approximately 0.0223 mol. Finally, we can calculate the mass of SO2 by multiplying the number of moles by the molar mass, which gives us approximately 1.427 g.

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  • 3. 

    A necklace has 6 g of diamond in it. What are the number of atoms in it?

    • A.

      6.02 x 1023

    • B.

      12.04 x 1023

    • C.

      1.003 x 1023

    • D.

      3.01 x 1023

    Correct Answer
    D. 3.01 x 1023
    Explanation
    The answer, 3.01 x 10^23, is the correct option because it represents Avogadro's number, which is the number of atoms or molecules in one mole of a substance. In this case, since the necklace contains 6g of diamond, which has a molar mass of approximately 12g/mol, we can use the formula: number of atoms = (mass of substance / molar mass) x Avogadro's number. Plugging in the values, we get (6g / 12g/mol) x 6.02 x 10^23, which simplifies to 3.01 x 10^23 atoms.

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  • 4. 

    What is the mass of aluminum in 204 g of the aluminum oxide, Al2O3?

    • A.

      26 g

    • B.

      27 g

    • C.

      54 g

    • D.

      108 g

    Correct Answer
    D. 108 g
    Explanation
    The molar mass of Al2O3 is 102 g/mol. To find the mass of aluminum in 204 g of Al2O3, we need to calculate the mass of one mole of Al2O3 and then divide it by the molar mass of aluminum. Since there are 2 moles of aluminum in one mole of Al2O3, the mass of aluminum is 2 times the molar mass of aluminum. Therefore, the mass of aluminum in 204 g of Al2O3 is 2 * (26.98 g/mol) = 108 g.

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  • 5. 

    The reactant which is consumed earlier and gives least quantity of product is called

    • A.

      Reactant in excess

    • B.

      Stoichiometry

    • C.

      Limiting reactant

    • D.

      Stoichiometric amount

    Correct Answer
    C. Limiting reactant
    Explanation
    The limiting reactant is the reactant that is completely consumed in a chemical reaction, thereby limiting the amount of product that can be formed. It determines the maximum amount of product that can be obtained. In contrast, the reactant in excess is the reactant that is present in greater quantity than required for the reaction and is not completely consumed. The term "stoichiometry" refers to the quantitative relationship between reactants and products in a chemical reaction, while "stoichiometric amount" refers to the exact amount of reactants required for a reaction based on the stoichiometry.

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  • 6. 

    Which one of the following compounds contains the highest percentage by the mass of nitrogen

    • A.

      NH3

    • B.

      N2H4

    • C.

      NO

    • D.

      NH2OH

    Correct Answer
    B. N2H4
    Explanation
    N2H4 contains the highest percentage by mass of nitrogen because it has two nitrogen atoms in its formula, compared to only one nitrogen atom in the other compounds. Since the percentage by mass is calculated by dividing the mass of nitrogen in the compound by the total mass of the compound and multiplying by 100, having two nitrogen atoms in N2H4 increases the numerator and thus the percentage of nitrogen in the compound.

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  • 7. 

    Vitamin-A has a molecular formula C20H30O. The number of vitamin-A molecules in 500 mg of its capsule will be?

    • A.

      6.02 x 1023

    • B.

      1.05 x 1021

    • C.

      3.01 x 1022

    • D.

      3.01 x 1023

    Correct Answer
    B. 1.05 x 1021
    Explanation
    The molecular formula of Vitamin-A is C20H30O, which means that it contains 20 carbon atoms, 30 hydrogen atoms, and 1 oxygen atom. To calculate the number of molecules in 500 mg of its capsule, we need to convert the mass of the capsule to moles using the molar mass of Vitamin-A. The molar mass of Vitamin-A can be calculated by adding the atomic masses of carbon, hydrogen, and oxygen. Once we have the number of moles, we can use Avogadro's number (6.02 x 10^23) to calculate the number of molecules. The correct answer, 1.05 x 10^21, is obtained by correctly performing these calculations.

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  • 8. 

    When one mole of each of the following is completely burnt in oxygen, which will give the largest mass of CO2?

    • A.

      Carbon monoxide

    • B.

      Diamond

    • C.

      Ethane

    • D.

      Methane

    Correct Answer
    C. Ethane
    Explanation
    When one mole of each substance is burnt in oxygen, the substance that will produce the largest mass of CO2 is ethane. This is because ethane (C2H6) has two carbon atoms, while the other substances have only one carbon atom. Since the number of carbon atoms directly affects the amount of CO2 produced, ethane will yield a larger mass of CO2 compared to the other substances.

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  • 9. 

    One mole of ethanol and one mole of ethane have an equal

    • A.

      Mass

    • B.

      Number of atoms

    • C.

      Number of electron

    • D.

      Number of molecules

    Correct Answer
    D. Number of molecules
    Explanation
    The correct answer is "Number of molecules." One mole of any substance contains Avogadro's number of particles, which is approximately 6.022 x 10^23. Therefore, both one mole of ethanol and one mole of ethane would have the same number of molecules, which is equal to Avogadro's number.

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  • 10. 

    Methane reacts with steam to form H2 and CO as shown below. What volume of H can be obtained from 100 cmof methane at the standard temperature and pressure?

    • A.

      300 cm3

    • B.

      200 cm3

    • C.

      150 cm3

    • D.

      100 cm3

    Correct Answer
    A. 300 cm3
    Explanation
    When methane reacts with steam, it produces hydrogen gas (H2) and carbon monoxide (CO). The question asks for the volume of hydrogen gas that can be obtained from 100 cm3 of methane at standard temperature and pressure. Since the reaction is stoichiometric, it means that for every molecule of methane, one molecule of hydrogen gas is produced. Therefore, the volume of hydrogen gas obtained will be equal to the volume of methane used, which is 100 cm3.

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  • 11. 

    The Avogadro's constant is the number of?

    • A.

      Atoms in 12 grams of carbon-12

    • B.

      Molecules in 1 mole of a substance

    • C.

      Electrons in 1 gram of hydrogen

    • D.

      Protons in 1 mole of a substance

    Correct Answer
    B. Molecules in 1 mole of a substance
    Explanation
    Avogadro's constant (6.022 × 10^23 mol-1) represents the number of particles, specifically molecules or atoms, in one mole of a substance. This constant allows chemists to relate the mass of a substance to the number of particles it contains. Option A is incorrect because it refers to the number of atoms in 12 grams of carbon-12, which is technically Avogadro's number (6.022 × 1023 atoms/mol), but it represents a specific isotope of carbon. Option C is incorrect because it refers to the number of electrons in 1 gram of hydrogen, which is unrelated to Avogadro's constant. Option D is incorrect because it mentions protons, whereas Avogadro's constant is associated with the number of molecules or atoms, not protons. 

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  • 12. 

    How many mole of oxygen are needed for the complete combustion of two moles of butane?

    • A.

      2

    • B.

      8

    • C.

      10

    • D.

      13

    Correct Answer
    D. 13
    Explanation
    The complete combustion of butane (C4H10) requires 13 moles of oxygen. This can be determined by balancing the chemical equation for the combustion of butane, which is C4H10 + 13O2 -> 8CO2 + 10H2O. The equation shows that for every 1 mole of butane, 13 moles of oxygen are needed to produce 8 moles of carbon dioxide and 10 moles of water. Therefore, for 2 moles of butane, we would need 2 x 13 = 26 moles of oxygen.

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  • 13. 

    If four moles of SO2 are oxidized to SO, how many moles of oxygen molecules are required?

    • A.

      0.5

    • B.

      1.0

    • C.

      1.5

    • D.

      2.0

    Correct Answer
    D. 2.0
    Explanation
    When four moles of SO2 are oxidized to SO3, the balanced chemical equation shows that two moles of SO2 react with one mole of O2 to produce two moles of SO3. Therefore, to oxidize four moles of SO2, we would need two moles of O2.

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  • 14. 

    What is the mass of 2 moles of chlorine gas if the relative atomic mass of chlorine is 35.5 amu?

    • A.

      142 g

    • B.

      71 g

    • C.

      35.5 g

    • D.

      18.75 g

    Correct Answer
    B. 71 g
    Explanation
    The molar mass of chlorine gas (Cl2) is equal to the sum of the atomic masses of two chlorine atoms. Since the relative atomic mass of chlorine is 35.5 amu, the molar mass of chlorine gas is 2 * 35.5 = 71 g.

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  • 15. 

    Which of the following statements is incorrect?

    • A.

      12 g of carbon gas contains one mole of atoms

    • B.

      28 g of nitrogen gas contains one mole of molecules of N2

    • C.

      1dmof 1.0 mole dm-3 solution of NaCl contains one mole of chloride ions

    • D.

      None of above

    Correct Answer
    D. None of above
    Explanation
    The given question asks for the incorrect statement among the options. The correct answer is "None of above," which means that all of the statements are correct. This implies that 12 g of carbon gas does contain one mole of atoms, 28 g of nitrogen gas contains one mole of molecules of N2, and 1 dm3 of 1.0 mole dm-3 solution of NaCl does contain one mole of chloride ions.

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  • 16. 

    One mole of propane has the same

    • A.

      Number of H- atoms as one mole of methane (CH4)

    • B.

      Number of C-atoms as in one mole of butane (C4H10)

    • C.

      Mass as half a mole of hexane (C6H14)

    • D.

      Number of molecules as in one mole of ethane (C2H6)

    Correct Answer
    A. Number of H- atoms as one mole of methane (CH4)
    Explanation
    One mole of propane (C₃H₈) contains the same number of hydrogen atoms as one mole of methane (CH₄). Both molecules have four hydrogen atoms. This equality arises from the stoichiometry of the compounds, where each carbon atom bonds with four hydrogen atoms in the respective molecules.

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  • 17. 

    What is the mass of one mole of iodine molecules?

    • A.

      254 g

    • B.

      74 g

    • C.

      106 g

    • D.

      127 g

    Correct Answer
    A. 254 g
    Explanation
    One mole of any substance is equal to its molar mass in grams. The molar mass of iodine (I2) is approximately 254 g/mol. Therefore, the mass of one mole of iodine molecules is 254 g.

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  • 18. 

    What volume of SO2 at room temperature and pressure is produced on heating 9.7 g of Zinc sulphide (ZnS) if reaction takes place as follows?

    • A.

      3.2 liters

    • B.

      4.2 liters

    • C.

      1.6 liters

    • D.

      2.38 liters

    • E.

      None of these

    Correct Answer
    D. 2.38 liters
Janyce Wowk |BS (Chemistry) |
Chemistry
Janyce is a chemistry professional with a B.S. in Chemistry from Montclair State University. Her experience as a research assistant and lab technician in a PFAS laboratory has allowed her to develop strong laboratory, data analysis, and research skills. On our review board team, Janyce reviews chemistry quizzes, ensuring accuracy and enhancing the quality of our educational materials. Her chemistry expertise and commitment to precision make her a valuable asset in maintaining high-quality resources for learners.

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  • Jul 03, 2024
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