NVCC AL Campus CHM 111 Worksheet
Chapter 4: Chemical quantities and aqueous solutions
Q1.
Name: ______________________
Consider the following balanced reaction: 2 C4H10 (g) +13 O2 (g) → 8 CO2 (g) + 10 H2O (g)
a) How many moles of O2 are needed to completely react with 0.62 moles of C4H10?
4.0 mol O2
b) How many moles of CO2 can be produced from 0.62 moles of C4H10?
2.5 mol CO2
c)
How many moles of H2O can be produced from 0.62 moles of C4H10?
3.1 mol H2O
d) How many moles of O2 would have to react to produce 0.25 moles of CO2?
0.41 mol O2
Q2.
Consider the following balanced reaction: 2 Fe (s) + Al2O3 (s)  2 Al (s) + Fe2O3 (s)
If 6.25 moles of Fe react with 2.50 moles of Al2O3
a) Which reactant is the limiting reagent?
Al2O3
b) How many grams of Al are produced?
135 g Al
NVCC AL Campus CHM 111 Worksheet
Q3. Balance the reaction and complete the following table. Each row is its own question. For example; for row 1 you
should determine the grams of CH4 using the 1.00 moles of CH4, and then calculate the moles and grams of the
rest of the compounds. Show your work below the table.
_____CH4 + _____ O2
Molar Mass
______
Moles CH4
g CH4
1.00
16.0 g
→
_________
Moles O2
_____CO2 + _____ H2O
__________
g O2
Moles CO2
64.0 g
1.00 mol
16.5
11.9 g
Q4.
___________
g CO2
Moles H2O
36.0
11.3 g
32.8
What is the molarity of the solution prepared by diluting 122.5 ml of 0.225 M HCl to 750.0 ml?
0.0368M
Q5.
How many grams of Nickel (II) chloride are needed to prepare 100.0 ml of 0.125 M solution?
1.62 g
g H2O
NVCC AL Campus CHM 111 Worksheet
Q6. Complete and balance the following reactions. Write the corresponding complete and net ionic equations.
a) Hg2(NO3)2 (aq) +
b)
Ba(NO3)2 (aq) +
K2CO3 (aq) →
(NH4)2CO3 (aq)
→ BaCO3(s) + 2 NH4NO3(aq)
Ba2+(aq) + 2 NO3-(aq) + 2 NH42+(aq) + CO32-(aq)  BaCO3(s) + 2 NH42+(aq) + 2 NO3-(aq)
Ba2+(aq) + 2 CO32-(aq)  BaCO3(s)
c) Pb(NO3)2 (aq) +
d) K2SO3 (aq) +
e) HClO3 (aq) +
KI (aq) →
HCl (aq) →
→ H2O (l) + NaClO3(aq)
NaOH (aq)
H+(aq) + ClO3-(aq) + Na +(aq) + OH-(aq)  H2O (l) + K+(aq) + ClO32-(aq)
H+(aq) OH-(aq)  H2O (l)
f) Mg(NO3)2 (aq) +
K2SO4 (aq) →
NVCC AL Campus CHM 111 Worksheet
Q7.
Oxygen gas can be produced by the decomposition of KClO3
2KClO3 (s) → 2 KCl + 3 O2 (g)
How many grams of O2 can be produced from 1.625 g of KClO3 ?
0.6365 g
Q8.
Calculate the Molarity of the solution prepared by dissolving 26.0 g of Ammonium chloride in a total volume of
750.0 ml solution.
0.649 M
Q9.
What volume of 0.125 M KMnO4 (aq) solution can be prepared from 12.623 g of KMnO4?
0.639 L
NVCC AL Campus CHM 111 Worksheet
Q10. What volume of 0.125 M Na3PO4 is required to precipitate all the silver ions from 500.0 mL of 0.500 M
AgNO3? Write the balanced equation first!
0.667 L
Q11. 12.25 ml HCl (aq) solution was needed to completely neutralize 25.00 ml of 0.125 M KOH. What was the molarity
of the acid? Write down the balanced equation first!
0.255 M
NVCC AL Campus CHM 111 Worksheet
Q12.
a)
Complete and balance the following reactions:
Sulfuric acid reacts with aqueous strontium hydroxide
H2SO4(aq) + Sr(OH)2(aq)  2 H2O (l) + SrSO4(s)
b)
nitric acid reacts with aqueous potassium hydroxide
c) Aqueous solutions of Sodium carbonate and Copper (II) sulfate are mixed
Q13.
Consider the reaction for the manufacture of Aluminum sulfate:
2 AlCl3 (aq) + 3 H2SO4 (aq) → Al2(SO4)3(aq) + 6 HCl (aq)
a) If 15.0 g of AlCl3was mixed with 25.0 g of H2SO4, which reactant is the limiting reagent?
AlCl3
b) Calculate the theoretical yield of Al2(SO4)3.
19.2 g
c) If only 18.63 g of Al2(SO4)3 was produced, what is the percent yield of Al2(SO4)3?
97.0%
NVCC AL Campus CHM 111 Worksheet
Q14. Balance the following reaction
______ C2H6 + ______ O2 → _______ CO2 + _______ H2O
Complete the following table based on the balanced chemical reaction above. (Each row is its own calculation). Show
your work below the table.
moles of
C2H6
grams of
C2H6
2.00
moles of
O2
grams of
O2
Limiting
reagent
Grams of reagent
in excess
Grams of CO2
produced
C2H6
32 g
176 g
8.00
1.66
3.13
50.0
O2
100