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WorksheetsChemistry Exam
Total questions: 65
Worksheet time: 2hrs 24mins
Name
Class
Date
1.
What is the molar mass of Ca(NO3)2?
a)
164.03 g/mole
b)
228.32 g/mole
c)
150.02 g/mole
d)
218.05 g/mole
2.
What is the molar mass of B2(CO3)3?
a)
81.632 g/mol
b)
94.842 g/mol
c)
38.822 g/mol
d)
201.648 g/mol
3.
How many moles of molecules of F2 in 18 x 1023 molecules of F2 ?
a)
18 x 1023 / 6 x 1023
b)
18 x 1023 / 2
c)
18 x 1023 x 6 x 1023
4.
How many liters of gas are there in 44 g of bromine gas at STP?
a)
3.5 L
b)
10.54 L
c)
12.34 L
d)
6.17 L
5.
What is the mass of 6.7 moles of H2O?
a)
110 g
b)
120 g/mol
c)
120 g
d)
120 mol
6.
A container with a volume of 893 L contains how many moles of air at STP?
a)
20003.2 L
b)
39.9 L
c)
22.4 L
d)
none of the choices
7.
Balance this equation: ___Al2O3 ---> ___Al + ___O2
a)
Cannot be balanced
b)
2Al2O3 ---> 2Al + 3O2
c)
2Al2O3 ---> 4Al + 3O2
d)
3Al2O3 ---> 2Al + O2
8.
Balance this equation:
__Li + __Cl2 -> __LiCl
__Li + __Cl2 -> __LiCl
a)
2Li + Cl2 -> 4LiCl2
b)
2Li + Cl2 -> LiCl2
c)
2Li + 1Cl2 -> 2LiCl
d)
Not possible to balance
9.
Use the following equation:
NaIO3(aq) + 6HI(aq) --> 3I2(s) + NaI(aq) + 3H2O(l)
How many moles of I2 can be made from 6.55 moles of NaIO3?
NaIO3(aq) + 6HI(aq) --> 3I2(s) + NaI(aq) + 3H2O(l)
How many moles of I2 can be made from 6.55 moles of NaIO3?
a)
4.55 moles I2
b)
23.18 moles I2
c)
19.65 moles I2
d)
34.99 moles I2
10.
A gas at 7700.7 kPa occupies a volume of 768 mL. Calculate the volume at 23 kPa.
a)
260000 mL
b)
270000 mL
c)
250000 mL
d)
4257285689 mL
11.
A gas at 78oC occupies a volume of 345 ml. Calculate the volume at -228oC.
a)
44 mL
b)
45 mL
c)
43 mL
d)
42 mL
12.
A sample of oxygen gas occupies a volume of 2.5 L at 2 atm. What volume will it occupy at 1.25 atm pressure?
a)
4 atm
b)
4 L
c)
2 atm
d)
2 L
13.
A gas at 294 K occupies 2.34 L. At what temperature will the volume be 4.03 L?
a)
506.3 K
b)
506.3 L
c)
482.9 K
d)
482.9 L
14.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L
b)
7.81 L
c)
4.63 L
d)
4.36 L
15.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure.
a)
0 K
b)
107 K
c)
207 K
d)
307 K
16.
The following graph shows a ____ relationship.
a)
Direct
b)
Inverse
17.
The following graph shows the inverse relationship between _____
a)
Pressure and Volume
b)
Volume and Temperature
c)
Pressure and Temperature
d)
Volume and Moles
18.
All matter consists of tiny particles that are in constant motion is referred to as __________
a)
Kinetic Energy
b)
Kinetic molecular theory
c)
absolute zero
d)
Pressure
19.
A sample of iron receives 50.J of heat energy that raises the temperature of the iron 25.0°C. If iron has a specific heat of .10 J/g°C, what is the mass of the iron sample?
a)
25g
b)
30g
c)
20g
d)
50g
20.
What type of reaction is pictured behind?
a)
endothermic
b)
exothermic
21.
Endothermic reactions feel
a)
warm
b)
cold
22.
energy in endothermic reactions is
a)
released
b)
ended
c)
absorbed
23.
If 238 J of heat is absorbed by a sample of metal with a mass of 40.7 g, and it raises the temperature from 20.0°C to 32.4°C, what is the specific heat capacity of the metal?
a)
2.34 J/g°C
b)
0.472 J/g°C
c)
6.13 J/g°C
d)
0.163 J/g°C
24.
Energy can not be created or destroyed, it can only be transferred refers to the....
a)
law of conservation of energy
b)
law of conservation of mass
c)
life facts
d)
law of conservation of chemistry
25.
A liquid with a specific hear of 1.9 J/gC has 4750 J of energy added to it. The temperature changed from 20 degrees C to 30 degrees C, what is the mass of the liquid?
a)
250 cal
b)
2500cal
c)
250 g
d)
2500 cal
26.
Energy of motion is another name for
a)
kinetic energy.
b)
potential energy.
c)
thermal energy.
d)
radiant energy.
27.
When an object is dropped, the energy transformation is:
a)
thermal to kinetic
b)
potential to kinetic
c)
kinetic to potential
d)
mechanical to chemical
28.
Plants use photosynthesis to convert sunlight into sugar for food. This is an example of converting
a)
chemical energy to solar energy
b)
solar energy to chemical energy
c)
kinetic energy to potential energy
d)
potential energy to chemical energy
29.
When you rub your hands together on a cold day, you use friction to convert
a)
electrical into electromagnetic
b)
nuclear into electrical
c)
thermal into nuclear
d)
kinetic into thermal
30.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
31.
A solution with a pH of 3.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
32.
A solution with a pH of 8.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
33.
Ca(OH)2 is an example of a(n)
a)
Acid
b)
Base
c)
Neutral
34.
HBr is an example of a(n)
a)
Acid
b)
Base
c)
Neutral
35.
The pOH of sea water is 5.9. What is its pH? [pH = 14 - pOH]
a)
0.0000000083
b)
0.0000013
c)
5.9
d)
8.1
36.
The hydroxide ion is a soft drink is 5.00 x 10-12 M. Find the pH.
a)
0.002
b)
2.7
c)
11.3
d)
14
37.
The [H+] is orange juice is 0.00020 M. FInd the pH of orange juice.
a)
1
b)
3.7
c)
10.3
d)
13
38.
What is the name of H3PO4?
a)
hydrophosphoric acid
b)
phosphorous acid
c)
phosphoric acid
d)
phosphoric hydroxide
39.
What is the name of Mg(OH)2
a)
magnesium hydroxide acid
b)
hydromagnesium acid
c)
magnesium oxygen hydride
d)
magnesium hydroxide
40.
What is the formula of hydrosulfuric acid?
a)
H2S
b)
H2SO4
c)
HS
d)
HSO4
41.
What is the pH of a solution if [H+] = 6.0 x 10-10 M?
a)
3.45
b)
6.25
c)
9.22
d)
11.34
42.
Predict the products for the following reaction:
LiOH + H2SO4 -->
LiOH + H2SO4 -->
a)
LiSO4 + H2O
b)
LiSO4 + H2(OH)
c)
Li2SO4 + H2O
d)
Li2SO4 + H2(OH)
43.
NaC(aq) l + AgNO3(aq) --> NaNO3(aq) + AgCl(s)
a)
Acid/base (neutralization)
b)
Redox (reduction/oxidation)
c)
Precipitation
d)
Combustion
44.
Mg(s) + HC(aq) l --> MgCl2(aq) + H2(g)
a)
Redox (reduction/oxidation)
b)
Acid/base (neutralization)
c)
Combustion
d)
Precipitation
45.
Zn(s) + H2SO4(aq)--> ZnSO4(aq) + H2(g)
a)
Acid/base (neutralization)
b)
Redox (reduction/oxidation)
c)
Precipiation
d)
Decomposition
46.
NaOH(aq) + HCl(aq) --> NaCl(aq) + H2O(l)
a)
Double
b)
Single
c)
Decomposition
d)
Combustion
47.
A molecule with a positive end and a negative end is called a
a)
magnet
b)
polar molecule
c)
solution
d)
electrical molecule
48.
Which of the following would dissolve the slowest?
a)
a sugar cube in hot water
b)
a sugar cube in cool water
c)
powdered sugar in cool water
d)
powdered sugar in hot water
49.
What is the molarity of a solution that contains 0.3 moles of sugar in 2.5 liters of solution?
a)
8.33 m
b)
0.12 m
c)
0.12 M
d)
8.33 M
50.
When a solvent contains as much of the solute as it can hold, the solution is said to be
a)
supersaturated
b)
diluted
c)
saturated
d)
unsaturated
51.
How many L would you need to make a 1 M solution if you have 6 moles of NaOH?
a)
2
b)
3
c)
4
d)
6
52.
Use the solubility chart for: AgCl
a)
soluble
b)
insoluble
53.
Use the solubility chart for: NaCl
a)
soluble
b)
insoluble
54.
Use the solubility chart for: K2SO4
a)
soluble
b)
insoluble
55.
Use the solubility chart for: CaCO3
a)
soluble
b)
insoluble
56.
When 50 grams of potassium chloride, KCl, is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
57.
When 20 grams of sodium chloride, NaCl, is dissolved in 50 grams of water at 90 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
58.
When 40 grams of potassium nitrate, KNO3, is dissolved in 200 grams of water at 20 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
59.
Solution that contains less solute than a saturated solution under the same conditions
a)
Saturated
b)
unsaturated
c)
supersaturated
d)
solution
60.
What type of bonding occurs between water molecules?
a)
oxygen bonding
b)
hydrogen bonding
c)
water bonding
d)
nuclear bonding
61.
What property of water is responsible for a skilled chemistry student being able to float a paperclip on top of water?
a)
High surface tension
b)
Low surface tension
c)
High concentration
d)
Low concentration
62.
How many mL of 10.8M HCll are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
63.
What is the molarity of a solution made by adding 421.5 g of PbNO3 and adding water to 500. mL?
a)
300. M
b)
31.3 M
c)
3.13 M
d)
1.56 M
64.
How much 1.50M KBr can be made from 15.6 mL of concentrated KBr with a molarity of 9.65 M?
a)
150. mL
b)
151 mL
c)
1.00 L
d)
100. mL
65.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250. mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
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