Download Unit 8 Test Review

Name: _________________________________
Period: _______________
Unit 8 Test Review - ANSWERS
Define the following terms.
1.
Reactant – The starting substance in a chemical reaction.
2.
Product – A substance formed during a chemical reaction.
3.
Reagent – A substance used in a chemical reaction to detect, measure, examine, or produce other substances. Often used
interchangeably with reactant.
4.
Stoichiometry – The study of quantitative relationships between the amounts of reactants used and products formed by a chemical
reaction; is based on the law of conservation of mass
5.
Dimensional Analysis – A method of treating units as algebraic quantities, which can be cancelled.
6.
Limiting Reagent – A reactant that is totally consumed during a chemical reaction, limits the extent of the reaction, and determines the
amount of product
7.
Mole to Mole Ratio – In a balanced equation, the ratio between the numbers of moles of any two substances
8.
Activity Series of Metals – an invaluable aid to predicting the products of replacement reactions. Each element on the list
replaces from a compound any of the elements below it. The larger the interval between elements, the more vigorous the
reaction.
9.
Single replacement Reaction – A chemical reaction that occurs when the atoms of one element replace the atoms of another
element in a compound.
10. Coefficient – In a chemical equation, the number written in front of a reactant or product; tells the smallest number of particles of the
substance involved in the reaction
11. Subscripts - used in formulas to indicate the relative numbers of atoms of each type in the compound.
Perform the following calculations.
12. Provide the following mole to mole ratios using the equation given below.
2Na + 2H2O  2NaOH + H2
a. Sodium to hydrogen
2:1
b.
Water to sodium hydroxide
2:2
c.
Hydrogen to water
1:2
13. Perform the following calculations using the equation given below.
Al2(SO4)3 + Pb(NO3)2
Al(NO3)3 + Pb(SO4)
a.
Balance the equation.
Al2(SO4)3 + 3Pb(NO3)2
b.
2Al(NO3)3 + 3Pb(SO4)
A reaction uses 150 moles of aluminum sulfate, how many moles of aluminum nitrate will be produced if lead (II)
nitrate is in excess?
150 mol Al2(SO4)3 X
= 300 mol Al(NO3)3
Name: _________________________________
c.
Period: _______________
A reaction uses 5 grams of lead (II) nitrate, if aluminum sulfate is in excess, how many moles of lead (II) sulfate will
be generated?
5 g Pb(NO3)2 X
d.
X
= .015 mol or .02 mol Pb(SO4)
If 150 moles of lead (II) nitrate react with 175 moles of aluminum sulfate, how many moles of aluminum nitrate will
be produced? How many grams of lead (II) sulfate will be produced?
Part 1:
150 mol Pb(NO3)2 X
175 mol Al2(SO4)3 X
= 100 mol Al(NO3)3
= 117 mol Al(NO3)3
Part 2:
150 mol Pb(NO3)2 X
X
= 45489 g or 4.5 x 104 g Pb(SO4)
14. Write the steps describing how to balance a chemical equation. Making sure to use the following terms: coefficients and
subscripts.
Step 1: Write the unbalanced equation.



Chemical formulas of reactants are listed on the lefthand side of the equation.
Products are listed on the righthand side of the equation.
Reactants and products are separated by putting an arrow between them to show the direction of the reaction.
Reactions at equilibrium will have arrows facing both directions.
Step 2: Balance the equation.



Apply the Law of Conservation of Mass to get the same number of atoms of every element on each side of
the equation. Tip: Start by balancing an element that appears in only one reactant and product.
Once one element is balanced, proceed to balance another, and another, until all elements are balanced.
Balance chemical formulas by placing coefficients in front of them. Do not add subscripts, because this will
change the formulas.
Step 3: Indicate the states of matter of the reactants and products.





Use (g) for gaseous substances.
Use (s) for solids.
Use (l) for liquids.
Use (aq) for species in solution in water.
Write the state of matter immediately following the formula of the substance it describes.
15. What is the volume of 1 mole of a gas at STP?
22.4 L
16. What is STP?
Standard Temperature and Pressure : A temperature of 0°C and a pressure of 1 atmosphere (760 torr).
Name: _________________________________
Use the equation below to answer question 1.
NaHCO3 + HCl  NaCl + H2CO3
Period: _______________
1. If you use 3.2 moles of sodium bicarbonate, NaHCO3
a. how many moles of HCl would be used?
3.2 mol NaHCO3 X
= 3.2 mol HCl
b. how many moles of each product would be produced?
3.2 mol NaHCO3 X
= 3.2 mol NaCl
3.2 mol NaHCO3 X
= 3.2 mol H2CO3
Balance the equation below and use the reaction to answer question 2.
2 C8H18 + 25 O2  16 CO2 + 18 H2O
2. If you burn 4.33 moles of octane, C8H18.
a. what is the mass of oxygen required?
4.33 mol C8H18 X
= 1731.9 g or 1.73 x 103 g O2
X
b. how many grams of each product are produced?
4.33 mol C8H18 X
X
4.33 mol C8H18 X
X
= 1524.5 g or 1.52 x 103 g CO2
= 702 g H2O
Given the following equation, answer questions 3-4 below.
Cu + AgNO3  Ag + Cu(NO3)2
3. Balance the equation.
Cu + 2 AgNO3  2 Ag + Cu(NO3)2
4. If 170g of silver nitrate is consumed,
a. how many moles of silver are produced?
170 g AgNO3 X
X
= 1.00 mol Ag
b. how many grams of copper nitrate are produced?
170 g AgNO3 X
X
= 94g Cu(NO3)2
X
c. what is the mass of copper used?
170 g AgNO3 X
X
X
= 32 g Cu