Chapter 3 Chemistry Quiz

10 Questions | Attempts: 326

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Chapter 3 Chemistry Quiz - Quiz

While studying Chemistry, the chemical compounds and elements are some of the hardest concepts to understand. However, with a lot of exercises, it can be pretty easy. The Chemical quiz below tests on different reactions.


Questions and Answers
  • 1. 
    The atomic mass of copper is 63.55.  Given that there are only two naturally occurring isotopes of copper.   and , the naturally abundance of the  isotope must be approximately
    • A. 

      90%

    • B. 

      70%

    • C. 

      50%

    • D. 

      25%

    • E. 

      10%

  • 2. 
    A compound that contains only C and H was burned in excess oxygen.  The following masses were obtained after the complete combustion of the compound in oxygen:  22.0 g of and 18.0 g  was produced by the combustion.  Identify the correct empirical formula for the hydrocarbon.
    • A. 

      CH

    • B. 

      CH subscript 2

    • C. 

      CH subscript 3

    • D. 

      CH subscript 4

  • 3. 
    In 1.00 mol of potassium zirconium sulfate trihydrate, , there are  
    • A. 

      3 x 6.02 x 10 to the power of 23 hydrogen atoms

    • B. 

      6.02 x 10 to the power of 23 sulfur atoms

    • C. 

      4 x 6.02 x 10 to the power of 23 potassium atoms

    • D. 

      4 moles of oxygen atoms

    • E. 

      4 moles of zirconium atoms

  • 4. 
    What is the maximum number of moles of  that can be produced by the reaction of 0.40 mol of Al with 0.40 mol of 
    • A. 

      0.10 mol

    • B. 

      0.20 mol

    • C. 

      0.27 mol

    • D. 

      0.33 mol

    • E. 

      0.40 mol

  • 5. 
    ...  (g) + ...  (g) --> ...  (g) + ...  (g)When the equation for the reaction represented above is balanced and all coefficients are reduced to the lowest whole-number terms, the coefficient for  (g) is
    • A. 

      1

    • B. 

      2

    • C. 

      3

    • D. 

      5

    • E. 

      6

  • 6. 
    A sample of a compound contains 3.21 g of sulfur and 11.4 g of fluorine.  Which of the following represents the empirical formula of the compound?
    • A. 

      SF subscript 2

    • B. 

      SF subscript 3

    • C. 

      SF subscript 4

    • D. 

      SF subscript 5

    • E. 

      SF subscript 6

  • 7. 
    If 0.40 mol of  and 0.15 mol of  were to react as completely as possible to produce , what mass of reactant would remain?
    • A. 

      0.20 g of H subscript 2

    • B. 

      0.40 g of H subscript 2

    • C. 

      3.2 g of H subscript 2

    • D. 

      4.0 g of H subscript 2

    • E. 

      4.4 g of H subscript 2

  • 8. 
    How many carbon atoms are contained in 2.8 g of ?
    • A. 

      1.2 x 10 to the power of 23

    • B. 

      3.0 x 10 to the power of 23

    • C. 

      4.6 x 10 to the power of 23

    • D. 

      1.2 x 10 to the power of 24

    • E. 

      6.0 x 10 to the power of 23

  • 9. 
    ...  (s) + ...  (l) ...  (s)When the equation above is balanced and all coefficients are reduced to lowest whole-number terms, what is the coefficient of  (l)?
    • A. 

      1

    • B. 

      2

    • C. 

      3

    • D. 

      4

    • E. 

      5

  • 10. 
    In which of the following compounds is the mass ratio of chromium to oxygen closest to 1.62 to 1.00?
    • A. 

      CrO3

    • B. 

      CrO2

    • C. 

      CrO

    • D. 

      Cr2O

    • E. 

      Cr2O3

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