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Honors Unit 7 Test Version A

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

 3. 

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

 4. 

 a list of metals in order of decreasing reactivity
 

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

 5. 
In which of the following is the name and formula given correctly?
a.
tin (IV) fluoride, SnFmc005-1.jpg
b.
sodium oxide, NaO
c.
barium nitride, BaN
d.
cobaltous chloride, CoClmc005-2.jpg
 

 6. 
What are the coefficients that will balance the equation below?
Nmc006-1.jpg + Hmc006-2.jpg mc006-3.jpg NHmc006-4.jpg
a.
1, 3, 2
b.
1, 1, 2
c.
1, 3, 3
d.
3, 1, 2
 

 7. 
How many valence electrons are in a silicon atom?
a.
2
b.
6
c.
8
d.
4
 

 8. 
Which of the following factors contributes to the increase in atomic size within a group on the periodic table?
a.
fewer electrons in the highest occupied energy level
b.
an increase in size of the nucleus
c.
an increase in number of protons
d.
more energy levels as you go down a group
 

 9. 
In the reaction 2CO(g) + Omc009-1.jpg(g) ® 2COmc009-2.jpg(g), what is the ratio of moles of oxygen used to moles of COmc009-3.jpg produced?
a.
2:2
b.
2:1
c.
1:2
d.
1:1
 

 10. 
The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NOmc010-1.jpg is formed?
mc010-2.jpg
a.
2.00 g
b.
1.00 g
c.
2.88 g
d.
32.0 g
 

 11. 
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.
42.0 moles
d.
33.6 moles
 

 12. 
How many moles of aluminum are needed to react completely with 1.2 mol of FeO?
2Al(s) + 3FeO(s) ® 3Fe(s) + Almc012-1.jpgOmc012-2.jpg(s)
a.
0.8 mol
b.
1.6 mol
c.
2.4 mol
d.
1.2 mol
 

 13. 
In the chemical equation Hmc013-1.jpgOmc013-2.jpg(aq) ® Hmc013-3.jpgO(l) mc013-4.jpg Omc013-5.jpg(g), the mc013-6.jpg is a ____.
a.
solid
b.
reactant
c.
product
d.
catalyst
 

 14. 
Chemical equations must be balanced to satisfy
a.
the law of conservation of mass.
b.
the law of definite proportions.
c.
Avogadro’s principle.
d.
the law of multiple proportions.
 

 15. 
In order for the reaction 2Al mc015-1.jpg 6HCl mc015-2.jpg 2AlClmc015-3.jpg mc015-4.jpg 3Hmc015-5.jpg to occur, which of the following must be true?
a.
A precipitate must be formed.
b.
Al must be above H on the activity series.
c.
Heat must be supplied for the reaction.
d.
Al must be above Cl on the activity series.
 

 16. 
Which of the following compounds is NOT an ionic compound?
a.
NaCl
c.
MgBr2
b.
Li(NO3)
d.
CO2
 

 17. 
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 only.
d.
They are composed of anions and cations.
 

 18. 
One of the products when aqueous Namc018-1.jpgCOmc018-2.jpg reacts with aqueous Sn(NOmc018-3.jpg)mc018-4.jpg is
a.
Sn(COmc018-5.jpg)mc018-6.jpg
b.
NaSn
c.
CNOmc018-7.jpg
d.
NaNOmc018-8.jpg
 

 19. 
What are the missing coefficients for the skeleton equation below?
Almc019-1.jpg(SOmc019-2.jpg)mc019-3.jpg(aq) mc019-4.jpg KOH(aq) ® Al(OH)mc019-5.jpg(aq) mc019-6.jpg Kmc019-7.jpgSOmc019-8.jpg(aq)
a.
2, 12, 4, 6
b.
1, 6, 2, 3
c.
4, 6, 2, 3
d.
1, 3, 2, 3
 

 20. 
Which of the following is a balanced equation representing the decomposition of lead(IV) oxide?
a.
PbO mc020-1.jpg Pb mc020-2.jpg Omc020-3.jpg
b.
PbOmc020-4.jpg mc020-5.jpg Pb mc020-6.jpg Omc020-7.jpg
c.
PbOmc020-8.jpg mc020-9.jpg Pb mc020-10.jpg 2O
d.
Pbmc020-11.jpgO mc020-12.jpg 2Pb mc020-13.jpg O
 

 21. 
A neon sign is being made with 80 grams of neon.  How many atoms are contained the neon sign?
a.
1.20 x 1024 atoms
c.
2.40 x 1024 atoms
b.
4.80 x 1024 atoms
d.
6.02 x 1023 atoms
 

 22. 
What is the percent composition by mass of sulfur in the compound MgSO4 (gram-formula mass = 120. g/mol)?
a.
53 %
c.
46 %
b.
27 %
d.
20 %
 

 23. 
Which of the following is true about limiting and excess reagents?
a.
The amount of product is determined by the limiting reagent.
b.
The reactant that has the smallest given mass is 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. 
Which statement is true if 12 mol CO and 12 mol Femc024-1.jpgOmc024-2.jpg are allowed to react?
3CO(g) + Femc024-3.jpgOmc024-4.jpg(s) mc024-5.jpg 2Fe(s) + 3COmc024-6.jpg(g)
a.
The limiting reagent is Femc024-7.jpgOmc024-8.jpg and 24 mol Fe will be formed.
b.
The limiting reagent is Femc024-9.jpgOmc024-10.jpg and 36 mol COmc024-11.jpg will be formed.
c.
The limiting reagent is CO and 8.0 mol Fe will be formed.
d.
The limiting reagent is CO and 3.0 mol COmc024-12.jpg will be formed.
 

 25. 
How many moles of Hmc025-1.jpgPOmc025-2.jpg are produced when 71.0 g Pmc025-3.jpgOmc025-4.jpg reacts completely to form Hmc025-5.jpgPOmc025-6.jpg?
mc025-7.jpg
a.
16.0 mol
b.
4.00 mol
c.
0.063 5 mol
d.
1.00 mol
 

 26. 
What is the formula mass of calcium nitrate, Ca(NO3)2?
a.
150 g
c.
164 g
b.
102 g
d.
70.0 g
 

 27. 
In a double-replacement reaction, the
a.
reactants are two elements.
b.
products are always molecular.
c.
reactants are two ionic compounds.
d.
products are a new element and a new compound.
 

 28. 
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
 

 29. 
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.
22.4 L
c.
5.60 L
b.
44.8 L
d.
11.2 L
 

 30. 
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 Cmc030-1.jpgHmc030-2.jpgOmc030-3.jpg completely reacted with oxygen?
a.
11 g
b.
1.8 g
c.
1.5 g
d.
66 g
 

 31. 
Glucose, Cmc031-1.jpgHmc031-2.jpgOmc031-3.jpg, is a good source of food energy. When it reacts with oxygen, carbon dioxide and water are formed. How many liters of COmc031-4.jpg are produced when 126 g of glucose completely react with oxygen?
Cmc031-5.jpgHmc031-6.jpgOmc031-7.jpg(s) + 6Omc031-8.jpg(g) mc031-9.jpg 6COmc031-10.jpg(g) + 6Hmc031-11.jpgO(l) + 673 kcal
a.
94.1 L
b.
5.33 L
c.
15.7 L
d.
4.21 L
 

 32. 
How many grams of Hmc032-1.jpgPOmc032-2.jpg are produced when 10.0 moles of water react with an excess of Pmc032-3.jpgOmc032-4.jpg?
mc032-5.jpg
a.
147 g
b.
653 g
c.
6.7 g
d.
1.22 g
 

 33. 
In a combustion reaction, one of the reactants is
a.
nitrogen.
b.
hydrogen.
c.
oxygen.
d.
a metal.
 

 34. 
Why do atoms share electrons in covalent bonds?
a.
to attain a full valence energy level and become stable
b.
to become ions and attract each other
c.
to become more polar
d.
to increase their atomic numbers
 

 35. 
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.
32 g
c.
16 g
b.
48 g
d.
24 g
 

 36. 
What is the maximum number of grams of PHmc036-1.jpg that can be formed when 6.2 g of phosphorus reacts with 4.0 g of hydrogen to form PHmc036-2.jpg?
Pmc036-3.jpg(g) + 6Hmc036-4.jpg(g) mc036-5.jpg 4PHmc036-6.jpg(g)
a.
0.43 g
b.
6.8 g
c.
45 g
d.
270 g
 

 37. 
When the equation KClOmc037-1.jpg(s) mc037-2.jpg KCl(s) + Omc037-3.jpg(g) is balanced, the coefficient of KClO3 is
a.
2.
b.
1.
c.
3.
d.
4.
 



 
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