Chemistry

Chapters 8 & 9 Study Questions

 

1.  Sodium carbonate and iron(III) chloride react to form a precipitate.

      a)  Write a balanced molecular equation for this reaction.

      b)  Write a balanced complete ionic equation for this reaction.

      c)  Write a balanced net ionic equation for this reaction.

 

2.  Using a solubility table, decide whether a precipitate will form when the following solutions are mixed.  If a precipitate forms, write a net ionic equation for the reaction.

      a)  iron(III) nitrate and potassium hydroxide

      b)  ammonium chloride and lithium carbonate

      c)  sodium sulfide and nickel(II) sulfate

 

3.  For each of the following equations

            i.  indicate whether it is a combustion (C), synthesis (S), decomposition (D), single replacement (SR), or double displacement (DD)

            ii.  indicate which reactions are oxidation-reductions (OR), precipitations (P) or acid-base (AB) reactions.

            iii.  predict the products and record their formulas.  If no reaction occurs, write “NR.” (Use Tables as needed to help you decide if a reaction occurs.)

            iv.  balance the equation.

      a)  Li(s)  +  Cl2(g)   ®                                            b)  Sr(NO3)2(aq)  +  K2SO4(aq)   ®

      c)  C3H6(g)   +   O2(g)   ®                                     d)  CaCl2(aq)   +   NaNO3(aq)   ®

      e)  Fe(s)   +  MgSO4(aq)   ®                                 f)  KI(l)   ®

      g)  Al(s)   +   HCl(aq)   ®                                      h)  HNO3(aq)  +  KOH(aq)   ®

 

4.  Write a chemical equation for the ionization of iron(III) nitrate when it dissolves in water.

 

5.  Chromium reacts with hydrochloric acid in a single replacement reaction.  The balanced equation is:

                                    2 Cr(s)  +  6 HCl(aq)   ®   2 CrCl3(aq)  +  3 H2(g)

 

      a)  How many moles of HCl are needed to produce 1.60 moles of CrCl3?

      b)  How many grams of chromium are required to react with 0.450 moles of HCl?

      c)  How many atoms of chromium are required to produce 12 moles of H2?

      d)  How many grams of Cr are needed to produce 3.20 g H2?

      e)  In an experiment, 10.2 grams of CrCl3 are produced starting from 8.30 grams of HCl.  What was the theoretical yield and the percent yield in this experiment?

      f)  When 6.0 moles of Cr are combined with 12.0 moles of HCl, which reactant is limiting?  How many moles of excess reactant are left over?

      g)  How many grams of CrCl3 are produced starting from 13.0 g of Cr and 43.8 g of HCl?

 

 

 

Summary of Chapter 8: Reactions in Aqueous Solutions

 

predicting whether a reaction will occur

precipitation reactions

strong electrolytes

using a solubility table

predicting whether a precipitate occurs

writing equations for precipitation reactions

molecular equations

complete ionic equations

net ionic equations

acids, bases

acid-base reactions

common strong acids

common strong bases

double displacement reactions

            precipitation reactions

            acid-base reactions

oxidation-reduction reactions

            synthesis (combination)

            decomposition

            combustion reactions

            single replacement reactions

 

 

Summary of Chapter 9:  Chemical Quantities

 

interpreting balanced chemical equations

stoichiometric calculations:

mole relationships between reactants and products

mass relationships between reactants and products

limiting reactant

theoretical yield

experimental yield

calculating percent yield