Ultimate Quiz On Stoichiometry Quiz

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  • 1/8 Questions

    Mole ratios for a reaction are obtained from the

    • Coefficients
    • Chemical symbols
    • Molar masses
    • Subscripts
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About This Quiz

The Ultimate Quiz on Stoichiometry tests understanding of mole ratios, reaction equations, and mass calculations. Participants apply chemical principles to solve stoichiometric problems, enhancing skills crucial for academic and professional success in chemistry.

Ultimate Quiz On Stoichiometry Quiz - Quiz

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  • 2. 

    Determine the mole ratio necessary to convert mole of aluminum to moles of aluminum chloride.  The balanced equation is 2AL + 3Cl2 → 2AlCl3

    • 2:3

    • 2:2

    • 3:2

    Correct Answer
    A. 2:2
    Explanation
    The balanced equation shows that for every 2 moles of aluminum (2AL), 2 moles of aluminum chloride (2AlCl3) are formed. Therefore, the mole ratio necessary to convert moles of aluminum to moles of aluminum chloride is 2:2.

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  • 3. 

    Using this balanced equation, 2C + FeCr2O4 → FeCr2 + 2CO2, what mole ratio would you use to convert moles of FeCr2O4 to moles of FeCr2?

    • 1:1

    • 2:1

    • 2:2

    Correct Answer
    A. 1:1
    Explanation
    The given balanced equation shows that for every 2 moles of FeCr2O4, 2 moles of FeCr2 are produced. Therefore, the mole ratio to convert moles of FeCr2O4 to moles of FeCr2 is 1:1.

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  • 4. 

    If 5.5 mol calcium carbide (CaC2) reacts with an excess of water, how many moles of acetylene (C2H2) will be produced?  The balanced equation is as follows:  CaC2 + 2H2O → Ca(OH)2 + C2H2

    • 11.0 moles

    • 5.50 moles

    • 352.0 moles

    • 2.75 moles

    Correct Answer
    A. 5.50 moles
    Explanation
    When 5.5 moles of calcium carbide reacts with an excess of water, according to the balanced equation, it produces an equal number of moles of acetylene. Therefore, 5.5 moles of calcium carbide will produce 5.5 moles of acetylene.

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  • 5. 

    Use the following balanced equation to determine how many moles of CaCO3 can be dissolved in 0.0250 mol of HCl.  CaCO3 + 2HCl → CaCl2 + H2O + CO2

    • 0.0250 mol

    • 0.05 mol

    • 0.0125 mol

    • 2.5 mol

    Correct Answer
    A. 0.0125 mol
    Explanation
    The balanced equation shows that 1 mole of CaCO3 reacts with 2 moles of HCl. Therefore, if 0.0250 mol of HCl is present, only half of that amount (0.0125 mol) of CaCO3 can be dissolved.

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  • 6. 

    The balanced chemical equation for the reaction that is used to fuel rockets is N2H2 + H2O → N2 + 2H2O.  How many grams of N2H2 are needed to produce 10.0 mol nitrogen gas?

    • 15 g

    • 300 g

    • 30.03 g

    • Option 4

    Correct Answer
    A. 300 g
    Explanation
    In the balanced chemical equation, the stoichiometric ratio between N2H2 and N2 is 1:1. This means that for every 1 mol of N2H2, 1 mol of N2 is produced. Therefore, to produce 10.0 mol of N2, we would need an equal amount of N2H2. The molar mass of N2H2 is 30.03 g/mol, so 10.0 mol of N2H2 would weigh 10.0 mol * 30.03 g/mol = 300 g.

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  • 7. 

    Chloroform (CHCl3) is produced by a reaction between methane and chlorine.  Use the balanced chemical equation for this reaction to determine the mass of CH4 needed to produce 50.0 g of CHCl3. Balanced Equation:  CH4 + 3Cl2 → CHCl3 + 3HCl

    • 6.72 grams

    • 119.37 grams

    • 10.04 grams

    • 11.9 grams

    Correct Answer
    A. 6.72 grams
    Explanation
    Based on the balanced chemical equation, 1 mole of CH4 reacts with 1 mole of CHCl3. To determine the mass of CH4 needed to produce 50.0 g of CHCl3, we need to convert grams of CHCl3 to moles using its molar mass (119.37 g/mol).

    50.0 g CHCl3 * (1 mol CHCl3 / 119.37 g CHCl3) * (1 mol CH4 / 1 mol CHCl3) * (16.04 g CH4 / 1 mol CH4) = 6.72 g CH4

    Therefore, the mass of CH4 needed to produce 50.0 g of CHCl3 is 6.72 grams.

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  • 8. 

    Consider the following balanced equation.  C12H22O11 + 3O2 → 2H3C6H5O7 + 3H2O  Determine the mass of citric acid (H3C6H5O7) produced when 2.5 mol C12H22O11 is used.

    • 5.0 mol

    • 192.14 grams

    • 481 grams

    • 961 grams

    Correct Answer
    A. 961 grams
    Explanation
    The balanced equation shows that 1 mole of C12H22O11 produces 2 moles of H3C6H5O7. Therefore, 2.5 moles of C12H22O11 will produce 2.5 * 2 = 5 moles of H3C6H5O7.
    The molar mass of H3C6H5O7 is 192.14 g/mol. Therefore, the mass of 5 moles of H3C6H5O7 is 5 * 192.14 = 960.7 grams.  Rounded to the nearest whole number, the mass of citric acid produced is 961 grams.

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  • Jan 07, 2025
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  • Feb 11, 2014
    Quiz Created by
    Vbknipp
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