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Transcript
Name: _______________________________________
Period: __________
Study Guide: Stoichiometry
**YOUR ANSWERS MUST INCLUDE THE PROPER NUMBER OF SIG FIGS AND
COMPLETE UNITS IN ORDER TO RECEIVE CREDIT FOR THE PROBLEM.**
BALANCE THE FOLLOWING EQUATIONS TO USE IN QUESTIONS 5 – 14:
1. ____ Al + ____ O2  ____ Al2O3
2. ____ Cu + ____ AgNO3  ____ Ag + ____ Cu(NO3)2
3. ____ Zn + ____ HCl  ____ ZnCl2 + ____ H2
4. ____ Fe + ____ Cl2  ____ FeCl3
PERFORM THE FOLLOWING STOICHIOMETRIC CALCULATIONS:
5. Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen. How many
moles of HCl are required to produce 7.50 moles of ZnCl 2?
6. Copper metal reacts with silver nitrate to form silver and copper(II) nitrate. How many
grams of copper are required to form 250 g of silver?
7. When aluminum is burned in excess oxygen, aluminum oxide is produced. How many
grams of oxygen are required to produce 0.75 moles of Al 2O3?
8. How many grams of iron(III) chloride are produced when 15.3 g of iron react with
excess chlorine gas?
9. When 9.34 g of zinc react with excess hydrochloric acid how many grams of zinc
chloride will be produced?
PERFORM THE FOLLOWING LIMITING REACTANT PROBLEMS:
10. When 16.3 g of magnesium and 4.52 g of oxygen gas react, how many grams of
magnesium oxide will be formed? Identify the limiting and excess reactants.
2 Mg + O2  2 MgO
11. If 25.3 g of aluminum reacts with 25.3 g of copper(II) sulfate, how many grams of copper
are formed? Identify the limiting and excess reactants in this single replacement
reaction.
2 Al + 3 CuSO4  3 Cu + Al2(SO 4)3
12. Identify the limiting and excess reactants when 1.00 g of zinc reacts with 150 mL of
0.250M Pb(NO 3)2. How many grams of lead are formed in this single replacement
reaction?
Zn + Pb(NO3)2  Pb + Zn(NO3)2
13. If 24.5 g of iron are placed in 1.00 L of 0.25M HCl, how many grams of FeCl 2 are
obtained? Identify the limiting and excess reactants in this single replacement reaction.
Fe + 2 HCl  FeCl2 + H2
PERFORM THE FOLLOWING PERCENT YIELD CALCULATIONS:
14. If 5.45 g of potassium chlorate are decomposed to form potassium chloride, 1.75 g of
oxygen gas are also given off. Find the theoretical and percent yields.
2 KClO3  2 KCl + 3 O2
Stoichiometry Review – Ch. 9
ANSWER KEY
BALANCED EQUATIONS
1. 4 Al + 3 O2  2 Al2O3
2. Cu + 2 AgNO3  2 Ag + Cu(NO3) 2
3. Zn + 2 HCl  ZnCl2 + H2
4. 2 Fe + 3 Cl2  2 FeCl3
STOICHIOMETRIC CALCULATIONS
5. 15.0 mol HCl
6. 74 g Cu
7. 36 g O2
8. 44.4 g FeCl 3
9. 19.5 g ZnCl2
LIMITING REACTANT
10. LR: O2
XS: Mg
Product: 11.4 g MgO
11. LR: CuSO4
XS: Al
Product: 10.0 g Cu
12. LR: Zn
XS: Pb(NO3)2
Product: 3.17 g Pb
13. LR: HCl
XS: Fe
Product: 16 g FeCl2
PERCENT YIELD
14. Theoretical: 2.13 g O2
Percent Yield: 82.2%
Chemical Reactions Review
IDENTIFY THE TYPE OF REACTION AND BALANCE THE EQUATION:
1. Sb + I2  SbI3
5. AlCl3 + Na2CO3  Al2(CO3)3 + NaCl
2. Li + H2O  LiOH + H2
6. HNO3 + Ba(OH)2  Ba(NO3)2 + H2O
3. AlCl3  Al + Cl2
7. Al + Pb(NO3)2  Al(NO3)3 + Pb
4. C6H12 + O2 CO2 + H2O
IDENTIFY THE TYPE OF REACTION & WRITE A BALANCED EQUATION (INCL. STATES):
8. Aqueous solutions of ammonium chloride and lead(II) nitrate produce lead(II) chloride
precipitate and aqueous ammonium nitrate.
9. Solid carbon disulfide burns in oxygen to yield carbon dioxide and sulfur dioxide gases.
10. Iron metal reacts with aqueous silver nitrate to produce aqueous iron(III) nitrate and
silver metal.
IDENTIFY THE TYPE OF REACTION, PREDICT THE PRODUCTS (STATES NOT REQUIRED),
AND BALANCE THE EQUATION:
11. Al(s) + NaOH(aq) 
12. C2H4(g) + O2(g) 
13. FeCl2(aq)+ K2S(aq) 
14. Ba(s) + O2(g) 
15. NH4NO3(aq) + NaCl(aq) 
16. SO2(g) 
17. Magnesium metal is added to aqueous hydrochloric acid.
18. Potassium metal is combined with chlorine gas.
19. Aqueous solutions of potassium bromide and silver nitrate are combined.
Chemical Reactions Review
ANSWER KEY
1. synthesis
2Sb + 3I2  2SbI3
2.
3.
4.
5.
6.
7.
single replacement
decomposition
combustion
double replacement
double replacement
single replacement
2Li + 2H2O  2LiOH + H2
2AlCl3  2Al + 3Cl2
C6H12 + 9O2  6CO 2 + 6H2O
2AlCl3 + 3Na2CO3  Al2(CO 3)3 + 6NaCl
2HNO3 + Ba(OH)2  Ba(NO3)2 + 2H2O
2Al + 3Pb(NO3)2  2Al(NO3)3 + 3Pb
8.
9.
10.
11.
12.
13.
double replacement
combustion
single replacement
single replacement
combustion
double replacement
2NH4Cl(aq) + Pb(NO3)2(aq)  PbCl2(s) + 2NH4NO3(aq)
CS2(s) + 3O2(g)  CO2(g) + 2SO2(g)
Fe(s) + 3AgNO 3(aq)  Fe(NO3 )3(aq) + 3Ag(s)
Al(s) + NaOH(aq)  N.R.
C2H4(g)+ 3O2(g)  2CO2(g) + 2H2O(g)
FeCl2(aq)+ K2S(aq)  FeS(s) + 2KCl(aq)
14.
15.
16.
17.
18.
comb, synthesis
double replacement
decomposition
single replacement
synthesis
2Ba(s) + O2 (g)  2BaO(s)
NH4NO3(aq) + NaCl(aq)  N.R.
SO2(g)  S(s) + O2 (g)
Mg(s) + 2HCl(aq)  MgCl2(aq) + H 2(g)
2K(s) + Cl2(g)  2KCl(s)
19. double replacement
KBr(aq) + AgNO3 (aq)  AgBr(s) + KNO3(aq)