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6.14.2: Types of Reactions (Exercises)

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    These are homework exercises to accompany the Textmap created for "Chemistry" by OpenStax. Some have been modified and added by Kristina Novek.

     

    Types of Chemical Reactions Exercises

     

    1.      Write a balanced molecular equation describing each of the following chemical reactions.

    a.  Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas.

    b.  Gaseous butane, C4H10, reacts with diatomic oxygen gas to yield gaseous carbon dioxide and water vapor.

    c.  Aqueous solutions of magnesium chloride and sodium hydroxide react to produce solid magnesium hydroxide and aqueous sodium chloride.

    d.  Water vapor reacts with sodium metal to produce solid sodium hydroxide and hydrogen gas.

     

    2.      Colorful fireworks often involve the decomposition of barium nitrate and potassium chlorate and the reaction of the metals magnesium, aluminum, and iron with oxygen.

    a.  Write the formulas of barium nitrate and potassium chlorate.

    b.  The decomposition of solid potassium chlorate leads to the formation of solid potassium chloride and diatomic oxygen gas. Write an equation for the reaction.

    c.  The decomposition of solid barium nitrate leads to the formation of solid barium oxide, diatomic nitrogen gas, and diatomic oxygen gas. Write an equation for the reaction.

     

    3.      Aqueous hydrogen fluoride (hydrofluoric acid) is used to etch glass and to analyze minerals for their silicon content. Hydrogen fluoride will     also react with sand (silicon dioxide).

    a.  Write an equation for the reaction of solid silicon dioxide with hydrofluoric acid to yield gaseous silicon tetrafluoride and liquid water.

    b.  Identify the type of reaction

     

    4.      Use the following equations to answer the questions.

    I.      H2O(s)  →  H2O(l)

    II.     CH3OH(g) + O2(g)  →  CO2(g)   +   H2O(g)

    III.    2H2O(l)  à  2H2(g) →  O2(g)

     

    a.  Which equation describes a physical change?

    b.  Which equation identifies the reactants and products of a combustion reaction?

    c.  Which equation is not balanced?

    d.  Which equation is a decomposition reaction?

     

    5. Indicate what type, or types, of reaction each of the following represents:

    a.  Ca(s)  +  Br2(l)  →  CaBr2(s)

    b.  Ca(OH)2(aq)  +  2 HBr(aq)  →  CaBr2(aq)  + 2 H2O(l)

    c.  C6H12(l)  +  9 O2(g)  →  6 CO2(g)  +  6 H2O(g)

    d.  Ca(s) + 2 H2O(l) → Ca(OH)2(aq) + H2(g)

     

    6. Indicate what type, or types, of reaction each of the following represents:

    a.  H2O(g) + C(s) → CO(g) + H2(g)

    b.  2 KClO3(s) → 2 KCl(s) + 3 O2(g)

    c.  Fe2O3 + 3 SO3 →  Fe2(SO4)3

    d.  Pb(NO3)2(aq) + H2SO4(aq) →  PbSO4(s)+ 2 HNO3(aq)

     

    7. Indicate what type, or types, of reaction each of the following represents:

    a.   3 Mg(s) + 2 AlPO4(aq) → 2 Al(s) + Mg3(PO4)2(aq)

    b.   CuCl2(aq) + 2 AgNO3(aq) → Cu(NO3)2(aq) + 2 AgCl(s)

    c.   CaI2(s) + Cl2(g) → CaCl2(s) + 2 I2(s)

    d.   CaCO3(s) →  CaO(s) + CO2(g)

    e.   KBr(aq) + AgNO3(aq) → KNO3(aq) + AgBr(s)

     

    8. Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

    a.      H3PO4

    b.      Al(OH)3

    c.      SeO2

    d.      KNO2

    e.      In2S3

    f.        P4O6

     

    9. Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

    a.      H2SO4

    b.      Ca(OH)2

    c.      BrOH

    d.      ClNO2

    e.      TiCl4

    f.        NaH

     

    10. In the following oxidation-reduction reactions, identify the species that are oxidized and reduced and the change in oxidation state for each:

    a.      2 Na(s) + 2 HCl(aq) →  2 NaCl(aq) + H2(g)

    b.      Mg(s) + Cl2(g) →  MgCl2(s)

    c.      K3P(s) + 2 O2(g) →  K3PO4(s)

    d.      C2H4(g) + 3 O2(g) → 2CO2(g) + 2H2O(g)

     

    11. In the following oxidation-reduction reactions, identify the species that are oxidized and reduced and the change in oxidation state for each:

    a.      Mg(s) + NiCl2(aq) →  MgCl2(aq) + Ni(s)

    b.      PCl3(l) + Cl2(g)  →  PCl5(s)

    c.      Zn(s) + H2SO4(aq) →  ZnSO4(aq) + H2(g)

     

     

     

     

    6.14.2: Types of Reactions (Exercises) is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts.

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