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Honors Unit 7 Test Version C

Matching
 
 
Match each item with the correct statement below.
a.
activity series of metals
c.
combustion reaction
b.
single-replacement reaction
d.
decomposition reaction
 

 1. 

 a reaction in which the atoms of one element replace the atoms of a second element in a compound
 

 2. 

 a list of metals in order of decreasing reactivity
 

 3. 

 a reaction in which a single compound is broken down into simpler substances
 

 4. 

 a reaction in which oxygen reacts with another substance, often producing heat or light
 

MC Identify the choice that best completes the statement or answers the question.
 

 5. 
Sulfur dioxide is the cause of acid rain and is common pollutant caused by volcanic eruptions, the burning of fossil fuels, and the exhaust from industrial facilities.  What is the mass in gram of 0.75 mole of SO2? (MM: 64.07 g/mol)
a.
16 g
c.
48 g
b.
32 g
d.
24 g
 

 6. 
Chemical equations must be balanced to satisfy
a.
the law of multiple proportions.
b.
the law of definite proportions.
c.
the law of conservation of mass.
d.
Avogadro’s principle.
 

 7. 
In the reaction 2CO(g) + Omc007-1.jpg(g) ® 2COmc007-2.jpg(g), what is the ratio of moles of oxygen used to moles of COmc007-3.jpg produced?
a.
1:2
b.
2:1
c.
1:1
d.
2:2
 

 8. 
When glucose is consumed, it reacts with oxygen in the body to produce carbon dioxide, water, and energy. How many grams of carbon dioxide would be produced if 45 g of Cmc008-1.jpgHmc008-2.jpgOmc008-3.jpg completely reacted with oxygen?
a.
11 g
b.
1.8 g
c.
66 g
d.
1.5 g
 

 9. 
Ethanol (C2H5OH) is used in hand sanatizer.  If 115 grams of C2H5OH is used to to make a batch of hand sanatizer, then how many moles are present in the batch? (MM: 46.08 g/mol)
a.
2.50 mol
c.
1.50 mol
b.
3.00 mol
d.
1.00 mol
 

 10. 
Glucose, Cmc010-1.jpgHmc010-2.jpgOmc010-3.jpg, is a good source of food energy. When it reacts with oxygen, carbon dioxide and water are formed. How many liters of COmc010-4.jpg are produced when 126 g of glucose completely react with oxygen?
Cmc010-5.jpgHmc010-6.jpgOmc010-7.jpg(s) + 6Omc010-8.jpg(g) mc010-9.jpg 6COmc010-10.jpg(g) + 6Hmc010-11.jpgO(l) + 673 kcal
a.
4.21 L
b.
94.1 L
c.
5.33 L
d.
15.7 L
 

 11. 
What are the coefficients that will balance the equation below?
Nmc011-1.jpg + Hmc011-2.jpg mc011-3.jpg NHmc011-4.jpg
a.
1, 1, 2
b.
3, 1, 2
c.
1, 3, 2
d.
1, 3, 3
 

 12. 
When the equation KClOmc012-1.jpg(s) mc012-2.jpg KCl(s) + Omc012-3.jpg(g) is balanced, the coefficient of KClO3 is
a.
1.
b.
2.
c.
3.
d.
4.
 

 13. 
Which of the following compounds is NOT an ionic compound?
a.
MgBr2
c.
Li(NO3)
b.
CO2
d.
NaCl
 

 14. 
Which statement is true if 12 mol CO and 12 mol Femc014-1.jpgOmc014-2.jpg are allowed to react?
3CO(g) + Femc014-3.jpgOmc014-4.jpg(s) mc014-5.jpg 2Fe(s) + 3COmc014-6.jpg(g)
a.
The limiting reagent is Femc014-7.jpgOmc014-8.jpg and 36 mol COmc014-9.jpg will be formed.
b.
The limiting reagent is CO and 8.0 mol Fe will be formed.
c.
The limiting reagent is CO and 3.0 mol COmc014-10.jpg will be formed.
d.
The limiting reagent is Femc014-11.jpgOmc014-12.jpg and 24 mol Fe will be formed.
 

 15. 
How many moles of Hmc015-1.jpgPOmc015-2.jpg are produced when 71.0 g Pmc015-3.jpgOmc015-4.jpg reacts completely to form Hmc015-5.jpgPOmc015-6.jpg?
mc015-7.jpg
a.
16.0 mol
b.
1.00 mol
c.
4.00 mol
d.
0.063 5 mol
 

 16. 
How many valence electrons are in a silicon atom?
a.
4
b.
6
c.
8
d.
2
 

 17. 
What is the formula mass of calcium nitrate, Ca(NO3)2?
a.
102 g
c.
70.0 g
b.
164 g
d.
150 g
 

 18. 
How many grams of Hmc018-1.jpgPOmc018-2.jpg are produced when 10.0 moles of water react with an excess of Pmc018-3.jpgOmc018-4.jpg?
mc018-5.jpg
a.
6.7 g
b.
147 g
c.
653 g
d.
1.22 g
 

 19. 
How many moles of aluminum are needed to react completely with 1.2 mol of FeO?
2Al(s) + 3FeO(s) ® 3Fe(s) + Almc019-1.jpgOmc019-2.jpg(s)
a.
2.4 mol
b.
1.6 mol
c.
0.8 mol
d.
1.2 mol
 

 20. 
What is the maximum number of grams of PHmc020-1.jpg that can be formed when 6.2 g of phosphorus reacts with 4.0 g of hydrogen to form PHmc020-2.jpg?
Pmc020-3.jpg(g) + 6Hmc020-4.jpg(g) mc020-5.jpg 4PHmc020-6.jpg(g)
a.
6.8 g
b.
45 g
c.
270 g
d.
0.43 g
 

 21. 
Which of the following factors contributes to the increase in atomic size within a group on the periodic table?
a.
an increase in size of the nucleus
b.
more energy levels as you go down a group
c.
fewer electrons in the highest occupied energy level
d.
an increase in number of protons
 

 22. 
Why do atoms share electrons in covalent bonds?
a.
to become more polar
b.
to increase their atomic numbers
c.
to become ions and attract each other
d.
to attain a full valence energy level and become stable
 

 23. 
Which of the following is true about limiting and excess reagents?
a.
The reactant that has the smallest given mass is the limiting reagent.
b.
The amount of product is determined by the limiting reagent.
c.
A balanced equation is not necessary to determine which reactant is the limiting reagent.
d.
Both reagents are left over after the reaction is complete.
 

 24. 
An environmental chemist is analyzing SO2 (MM: 64.07 g/mol) and has ordered a tank of the gas from a company who labled the tank as 16.0 grams of SO2.  The volume of the tank of SO2 (g)  at STP is closest to
a.
11.2 L
c.
22.4 L
b.
5.60 L
d.
44.8 L
 

 25. 
In a combustion reaction, one of the reactants is
a.
hydrogen.
b.
nitrogen.
c.
a metal.
d.
oxygen.
 

 26. 
In order for the reaction 2Al mc026-1.jpg 6HCl mc026-2.jpg 2AlClmc026-3.jpg mc026-4.jpg 3Hmc026-5.jpg to occur, which of the following must be true?
a.
A precipitate must be formed.
b.
Al must be above Cl on the activity series.
c.
Al must be above H on the activity series.
d.
Heat must be supplied for the reaction.
 

 27. 
What are the missing coefficients for the skeleton equation below?
Almc027-1.jpg(SOmc027-2.jpg)mc027-3.jpg(aq) mc027-4.jpg KOH(aq) ® Al(OH)mc027-5.jpg(aq) mc027-6.jpg Kmc027-7.jpgSOmc027-8.jpg(aq)
a.
4, 6, 2, 3
b.
1, 3, 2, 3
c.
1, 6, 2, 3
d.
2, 12, 4, 6
 

 28. 
In which of the following is the name and formula given correctly?
a.
tin (IV) fluoride, SnFmc028-1.jpg
b.
cobaltous chloride, CoClmc028-2.jpg
c.
barium nitride, BaN
d.
sodium oxide, NaO
 

 29. 
In a double-replacement reaction, the
a.
products are a new element and a new compound.
b.
reactants are two ionic compounds.
c.
reactants are two elements.
d.
products are always molecular.
 

 30. 
In the chemical equation Hmc030-1.jpgOmc030-2.jpg(aq) ® Hmc030-3.jpgO(l) mc030-4.jpg Omc030-5.jpg(g), the mc030-6.jpg is a ____.
a.
solid
b.
catalyst
c.
reactant
d.
product
 

 31. 
A neon sign is being made with 80 grams of neon.  How many atoms are contained the neon sign?
a.
4.80 x 1024 atoms
c.
2.40 x 1024 atoms
b.
1.20 x 1024 atoms
d.
6.02 x 1023 atoms
 

 32. 
Which of the following is true about the composition of ionic compounds?
a.
They are composed of cations only.
b.
They are formed from two or more nonmetallic elements.
c.
They are composed of anions and cations.
d.
They are composed of anions only.
 

 33. 
What is the percent composition by mass of sulfur in the compound MgSO4 (gram-formula mass = 120. g/mol)?
a.
20 %
c.
27 %
b.
53 %
d.
46 %
 

 34. 
The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NOmc034-1.jpg is formed?
mc034-2.jpg
a.
32.0 g
b.
1.00 g
c.
2.88 g
d.
2.00 g
 

 35. 
Which of the following is a balanced equation representing the decomposition of lead(IV) oxide?
a.
Pbmc035-1.jpgO mc035-2.jpg 2Pb mc035-3.jpg O
b.
PbO mc035-4.jpg Pb mc035-5.jpg Omc035-6.jpg
c.
PbOmc035-7.jpg mc035-8.jpg Pb mc035-9.jpg 2O
d.
PbOmc035-10.jpg mc035-11.jpg Pb mc035-12.jpg Omc035-13.jpg
 

 36. 
One of the products when aqueous Namc036-1.jpgCOmc036-2.jpg reacts with aqueous Sn(NOmc036-3.jpg)mc036-4.jpg is
a.
Sn(COmc036-5.jpg)mc036-6.jpg
b.
NaNOmc036-7.jpg
c.
CNOmc036-8.jpg
d.
NaSn
 

 37. 
A person attemps to fill their car tires with 9.03x1023 molecules of nitrogen gas (N2).  How many moles did the person attempt to put in the tires?
a.
1.50 moles
c.
0.667 moles
b.
33.6 moles
d.
42.0 moles
 



 
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