Ultimate Quiz On Stoichiometry Quiz

8 Questions | Attempts: 7770

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Ultimate Quiz On Stoichiometry Quiz - Quiz

Questions and Answers
  • 1. 
    Mole ratios for a reaction are obtained from the
    • A. 

      Coefficients

    • B. 

      Chemical symbols

    • C. 

      Molar masses

    • D. 

      Subscripts

  • 2. 
    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
    • A. 

      11.0 moles

    • B. 

      5.50 moles

    • C. 

      352.0 moles

    • D. 

      2.75 moles

  • 3. 
    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
    • A. 

      0.0250 mol

    • B. 

      0.05 mol

    • C. 

      0.0125 mol

    • D. 

      2.5 mol

  • 4. 
    Consider the following balanced equation.  C12H22O11 + 3O2 → 2H3C6H5O7 + 3H2O  Determine the mass of citric acid (H3C6H5O7) produced when 2.5 mol C12H22O11 is used.
    • A. 

      5.0 mol

    • B. 

      192.14 grams

    • C. 

      481 grams

    • D. 

      961 grams

  • 5. 
    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
    • A. 

      6.72 grams

    • B. 

      119.37 grams

    • C. 

      10.04 grams

    • D. 

      11.9 grams

  • 6. 
    Determine the mole ratio necessary to convert mole of aluminum to moles of aluminum chloride.  The balanced equation is 2AL + 3Cl2 → 2AlCl3
    • A. 

      2:3

    • B. 

      2:2

    • C. 

      3:2

  • 7. 
    Using this balanced equation, 2C + FeCr2O4 → FeCr2 + 2CO2, what mole ratio would you use to convert moles of FeCr2O4 to moles of FeCr2?
    • A. 

      1:1

    • B. 

      2:1

    • C. 

      2:2

  • 8. 
    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?
    • A. 

      15 g

    • B. 

      300 g

    • C. 

      30.03 g

    • D. 

      Option 4

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