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Chemistry 12: College Preparation Unit 1 Self Quiz - 1.14 - 1.17


Short Answer
 

 1. 
Classify each of the following reactions as a synthesis, decomposition, single displacement, or double displacement reaction:
a. CaO(s) + CO2(g) ® CaCO3(s)
b. FeS(s) + 2 HCl(aq) ® FeCl2(aq) + H2S(s)
c. Na2O(s) + CO2(g) ® Na2CO3(s)
d. 2 H2O(l) ® 2 H2(g) + O2(g)
e. 2 KCl(s) + 3 O2(g) ® 2 KClO3(s)
f. Fe(s) + Cu(NO3)2(aq) ® Fe(NO3)2(aq) + Cu(s)
g. Ba(ClO3)2(s) ® BaCl2(s) + 3 O2(g)
h. FeS(s) ® Fe(s) + S(s)
i. Cu(s) + 2 AgNO3(aq) ® 2 Ag(s) + Cu(NO3)2(aq)
j. 2 NaCl(aq) + H2SO4(aq) ® Na2SO4(aq) + 2 HCl(aq)
k. Ca(s) + 2 H2O(l) ® Ca(OH)2(aq) + H2(g)
 

 2. 
Using the solubility rules, complete each of the following double displacement reaction equations. Make sure that the equations are balanced. Write the total ionic equation and net ionic equation for each reaction. If no reaction occurs, write NR.
a. AgNO3(aq) + KCl(aq) ®
b. Pb(NO3)2(aq) + K2S(aq) ®
 

 3. 
Define each of the following terms:
a. solute
b. solvent
c. solubility
d. spectator ion
e. precipitate
f. supernate
 



 
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