Advanced Chemistry

Name: ______Date: ______Mods: ______

Ch. 8 Review

1)Identify each type of reaction by its general formula:

a.AB + CD  AD + CBreaction type: ______

b.CxHy + O2 CO2 + H2Oreaction type: ______

c.A + B  ABreaction type: ______

d.A + BC  AC + Breaction type: ______

e.AB  A + Breaction type: ______

2)Balance the equations below and identify the type of reaction:

  1. ____ K (s) + ____ MgBr2 (aq)  ____ KBr (aq) + ____ Mg (s)

reaction type: ______

  1. ____ HCl (aq) + ____ CaCO3 (s)  ____ CaCl2 (aq) + ____H2O (g) + ____ CO2 (g)

reaction type: ______

  1. ____ C8H18 (l) + ____ O2 (g)  ____ CO2 (g) + ____ H2O (g)

reaction type: ______

  1. ____ Ag2O (s)  ____ Ag (s) + ____O2 (g)

reaction type: ______

  1. ____ S8 (s) + ____O2 (g)  ____ SO3 (g)

reaction type: ______

  1. ____ C3H8 (l) + ____ O2 (g)  ____ CO2 (g) + ____ H2O (g)

reaction type: ______

  1. ____ AlBr3 (aq) + ____ K2SO4 (aq)  ____ KBr (aq) + ____ Al2(SO4)3 (aq)

reaction type: ______

  1. ____ CH4 (g) + ____ O2 (g)  ____ CO2 (g) + ____ H2O (g)

reaction type: ______

3)Write out balanced formula equations, including states of matter, from the following word equations:

  1. Aqueous solutions of sodium phosphate and calcium chloride react to form solid calcium phosphate and aqueous sodium chloride.
  1. Potassium metal and chlorine gas combine to form solid potassium chloride.

4)Double Replacement Reactions & Solubility Table: Predict the products (including states of matter) of the following double replacement reactions and balance the resulting equations. If a precipitate is formed, put a box around the precipitate. If all products are aqueous write NR, for nor reaction.

  1. ____Li2CO3 (aq) + ____AgNO3 (aq)
  1. ____(NH4)3PO4 (aq) + ____KCl(aq)
  1. ____Fe(C2H3O2)2 (aq) + ____Na2S (aq) 

5)Single Replacement Reactions & Activity Series: Determine if the following single replacement reaction can occur based on the activity series of metals. If the reaction can occur, predict the products (including states of matter) and balance the resulting equation. If a reaction cannot occur write NR, and move on.

  1. _____H2 (g) + _____KNO3 (aq) 
  2. _____Hg (s) + _____Mg(NO3)2 (aq) 
  3. _____Al (s) + _____ CaCl2 (aq) 
  4. _____Br2 (g) + _____CaI2 (aq) 
  5. _____Cr (s) + _____HCl (aq) 

6)Identify the type of chemical reaction, predict the products formed (including states of matter), and balance the resulting equation.

  1. ____ Na3PO4 (aq) + ____ CaCl2 (aq) 

reaction type: ______

  1. ____ Li (s) + ____ Br2 (g) 

reaction type: ______

  1. ____ NF3 (g) 

reaction type: ______

  1. ____ Fe(NO3)2 (aq) + ____ KOH (aq) 

reaction type: ______

  1. ____ Ni (s) + ____ HCl (aq) 

reaction type: ______

  1. ____ Pb(s) + ____ Cl2(g)

reaction type: ______

  1. ____ C5H12(l) + ____ O2(g)

reaction type: ______

  1. ____ MgBr2 (aq) + F2 (g) 

reaction type: ______

  1. ____ K3N (s) 

reaction type: ______

Ch. 8 - General Questions:

7)If all the following compounds were formed by double replacement reactions, which one would be considered a precipitate?

  1. potassium sulfatec. silver carbonate
  1. magnesium acetated. iron (II) nitrate

8)Which of the following metals is the least reactive?

  1. Nickelb. Copperc. Aluminum d. Tin

9)Which of the following coefficients correctly balances the equation below?

______C5H10O2 (l) + ______O2 (g)  ______CO2 (g) + ______H2O (g)

  1. 1, 7, 5, 5b. 1, 5, 5, 5 c. 2, 13, 10, 10 d. 2, 15, 10, 10

10)What is the law of conservation of mass and how does it relate to the balancing of equations?

11) Are the products found on the left or right hand side of a chemical equation?

12)Which state of matter is used when a soluble solid compound has been dissolved in water?

13)What does it mean if a chemical reaction has an arrow with a delta (Δ) sign over it?

14)Explain the difference between a coefficient and a subscript.