1.
Summer Assessment 2 (Chapters 3, 4, 5, 10, 11, 14 )
A reaction that results in forming one new substance is called:
a.
single replacement
c.
decomposition
b.
double replacement
d.
synthesis
2.
A reaction involving the breakup of a substance is called:
a.
combustion
c. synthesis
b.
single replacement
d. decomposition
3.
When the reaction Fe + Cl2
a.
1
b. 2
4.
5.
6.
-----------------FeCl3
The
reaction in question 3 is an example of:
a.
combustion
c.
synthesis
b.
single replacement
d.
decomposition
The
equation H3 PO4 + 3KOH --------- K3PO4 + 3H2O is an example of:
a.
b.
double replacement
single replacement
c.
d.
decomposition
synthesis
When the following equation is balanced, the coefficient in front of HC1 is:
Mg + HC1 ----- MgCl2 + H2
a. 6
b. 3
c. 1
7.
c. 3
is balanced, the coefficients for Cl2 is:
d. 4
d. 2
The equation in question 6 is an example of which type of reaction:
a.
synthesis
c.
decomposition
b.
single replacement
d.
double replacement
8.
The equation 2C3H7OH + 9O2 ------- 6CO2 + 8H2O is example of:
a.
combustion
c. double replacement
b.
single replacement
d. decomposition
9.
A symbol that is a triangle on the arrow in a chemical equation means:
a.
heat is supplied
c. yields
b.
a catalyst is needed
d. precipitate
10.
11.
In the reaction 6O2 +
is:
a. 1:2
b. 1:1
6H2O---- C6H12O + 6O2 the mole ratio of CO2 to C6H12O6
c. 6:1
d. 1:4
In the reaction C + 2H2 ----- CH4, the mole ratio of H2 to CH4 is.
a.
1:1
b. 2:1
c. 1:2
d. 2:4
12.
How many moles of SO3 are in 2.40x1024 molecules of SO3?
a. 0.250moles b. 4.00 moles
c. 3.40 x 1022 moles
d. 4.90 x 101 moles
13.
What is the mass of 0.400 moles of aspirin---C9H8O4?
a. 450 grams
b. 10.8 grams
c. 160. grams d. 72.0 grams
14.
What is the percent of carbon in C3H6O?
a. 20.7%
b. 62.1%
c. 1.61%
d. 30.0%
15.
Teflon contains 24.0% C and 76.0% F. What is the empirical formula?
a. C2F4
b. CF2
c. C12F38
d. C24F76
16.
The empirical formula of a compound is CH2F. The molecular mass of the compound is
66.0grams. The molecular formula of this compound is:
a. C4H8F4
b. C4H4F4
c. C2H4F2
d. CH2F
17.
For the reaction N2+ 3H2 —> 2NH3, how many moles of nitrogen are required to produce
18 moles of NH3.
a.
9
b. 18
c. 27
d. 36
18.
For the reaction 2CO + O2 -------- > 2CO2, how many moles of CO2 are obtained from
15 moles of oxygen?
a.
7.5
b. 15
c. 24
d. 30
Questions 19 and 20 refer to the following equation:
3Cu +
8HNO3 --------
3Cu(NO3)2 +
2NO
+
4H2O
19.
Calculate the number of moles of water produced when 6.6 moles of Cu(NO3)2 are
formed in the
reaction.
a.
4 moles
b. 6.6 moles
c. 4.9 moles
d. 8.8 moles
20.
How many grams of Cu would be needed to react with 4.00 moles HNO3?
a. 95.3g
b. 63.5g
c. 191g
d. 1.50g
21.
All of the following are basic assumptions of kinetic theory of gases except:
a.
matter is composed of very tiny particles
b.
c.
particles are in continual motion
collisions are elastic
d.
kinetic energy of particles remains constant
22. According to the kinetic molecular theory model explaining the properties of an ideal gas,
the average kinetic energy of gas particles is directly proportional to:
a. the volume of the individual particles
b. the attractive forces between gas particles
c. chemical composition of the gas particles
d. the Kelvin temperature
23. Unlike in an ideal gas, in a real gas,
a. particles have the same kinetic energy
c. the particles cannot diffuse
b. all particles move in the same direction
d. the particles exerts attractive forces on
each other
24. What does the constant bombardment of gas molecules against the inside walls of a
container produce?
a. temperature
b. density
c. pressure
d. diffusion
25.
The temperature at which the motion of particles ceases:
a. -273K
b. 0K
c. 0oC
d. 273oC
26.
Standard conditions when working with gases are defined as:
27.
a.
0K and latm
c.
00C and latm
b.
0K and lmmHg
d.
0oC and lmmHg
A pressure of 745mmHg is equal to:
a. 745 torr
b. 1 torr
c.1 pascal
d. 745 pascals
28.
An example of gas diffusion would be:
a.
filling a flat tire with air
b.
the odor of perfume spreading throughout the room
c.
a cylinder of oxygen stored under high pressure
d.
all of the above
29.
As the temperature of the gas in a balloon decreases:
a.
the volume increases
b.
the average kinetic energy of the gas decreases
c.
the pressure increases
d.
all of the above
30. With pressure constant the temperature of a gas is increased the volume will:
a. triple
b. decrease
c. remain the same
d. increase
31. A gas occupies a volume of 0.2L at 76mmHq. What volume will the gas occupy at
760mmHg?
a. 38L
b. 20L
c. 2L
d. 0.02L
32. A gas occupies 40.0L at –123oC. What volume does it occupy at 27oC?
a. 182 L
b. 8.80 L
c. 80.0 L
d. 20.0 L
33. A sample of gas at a pressure of 6.0atm at 50C. What is the new pressure if the
temperature rises to 35oC?
a. 5.4atm
b. 42atm
c. 6.6atm
d. 36atm
34. A gas has a volume of 120.L at 0.500atm and 15oC. What volume will it occupy at
0.250atm and10oC?
a. 240L
b. 244L
c. 236L
35. The molar volume of a gas at STP is:
a. 22.4mL
b. 20.4L
c. 22.4L
36.
d. 61.0L
d. 22,400L
The volume occupied by one mole of oxygen at STP is:
a. 11.2L
b. 22.4L
c. 16.0L
d. 32.0L
37. Calculate the volume of a 0.600mol gas at 15.0oC and a pressure of 1.10atm?
a. 12.9L
b. 22.4L
c. 24.6L
d. 129L
38. A sample of gas at 25oC has a volume of 11L and exerts a pressure of 660mmHg. How
many moles of gas are in the sample?
a.0.39mol
39.
b. 3.9mol
In the reaction C + O2 -----
a. l.5L
b. 0.5L
c. 2.0L
c. 9.3mol
CO2
d. 87mol
3.0L of O2 will yield what volume of CO2 at STP?
d. 3.0L
40. Water in air is an example of which solute-solvent combination?
a. gas-liquid
b. liquid-gas
c. liquid-liquid
d. gas-gas
41. Colloids:
a. can be separated by filtering
b. settles out when allowed to stand
c. scatter light
d. are heterogeneous
42. Which of the following decreases the average speed of solvent molecules?
a. increases temperature
b. stirring the solution
c. adding more solvent
d. decreasing the temperature
43. As temperature increases, solubility of gases in liquids:
a. increases
b. decreases
c. can increase or decrease
d. is not affected
44. What is the molarity of 200. ml of solution in which 2.0 moles of sodium bromide is
dissolved?
a. 2.0 M
b. 10. M
c. 0.040 M
d. 4.0 M
45. What is the percent by mass of a solution composed of 2.55g of acetone, CH3COCH3
dissolved in 200.g of water?
a. 0.000220%
b. 0.0126%
c. 0.1.26%
d. 1.28%
46. Acids generally release hydrogen gas when they react with:
a. nonmetals b. semimetals
c. active metals
d. inactive metals
47. According to the traditional definition an acid contains:
a. Hydrogen that does not ionize
b. Hydrogen that ionizes to H+ ions
c. Oxygen that does not ionize
d. Oxygen that ionizes to O2-ions
48. According to the traditional definition, bases produce what type of ions in solution?
a. hydronium
b. hydrogen
c. hydride
d. hydroxide
49. When a nonmetallic oxide such as sulfur dioxide combines with water, the resulting solution
would:
a. have a pH less than 7
b. have a pH greater than 7
c. be a base
d. have a pH of 7
50. The acid H2CO3 would decompose to yield what gas?
a. hydrogen
b. carbon
c. water vapor
d. carbon dioxide