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Adv. Chemistry - T.1 Final Exam. Revision Quiz # 2

Total questions: 60

Worksheet time: 3hrs 26mins

Name
Class
Date
1.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm (make sure you use the correct R value).
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
2.
You have a gas that has a pressure of 2 ATM and a volume of 10L.  What would be the new volume if the pressure was changed to 1 ATM?
a)
5 L
b)
20 L
c)
It would stay at 10L
d)
1 L
3.
A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC.  What is the new volume of the gas?
a)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
4.
A sample of oxygen gas has a volume of 150.0 mL when its pressure is .947 atm. What will the volume of the gas be if it is lowered to a pressure of 0.658 atm and the temperature remains constant?
a)
72 mL
b)
144 mL
c)
216 mL
d)
288 mL
5.
What is the formula for Boyle's Law?
a)
P1V1=P2V2
b)
P1V1/P2V2
c)
P1V2=P2V1
d)
P1/V1=P2/V2
6.
A gas occupies 4.98 L at 2.6 atm of pressure. What volume does it occupy at 1.8 atm pressure?
a)
12.9 L
b)
0.72 L
c)
7.2 L
d)
3.44 L
7.
A gas at a volume of 4 liters is at a pressure of 2 atm. The volume is changed to 16 Liters, what must the new pressure be?
a)
2 atm
b)
12 atm
c)
10 atm
d)
0.5 atm
8.
The relationship of which two variables are compared in Boyle's Law?
a)
pressure & volume
b)
volume & temperature
c)
temperature & pressure
d)
volume & moles (amount of gas)
9.
Records show that the incident of tire explosion is high during summer season.  Which of the following gives the best explanation for this observation?
a)
there are more travellers during summer vacation
b)
high temperature during summer season causes the air inside the tire to expand
c)
vehicles' tires are no well maintained
d)
there is too much air inside the tires
10.
Which of the following would increase the pressure on a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
11.

Temperature should always be expressed in Kelvin (K). If A 600 mL sample of nitrogen is heated from 27 °C to 77 °C at constant pressure. What is the final volume of nitrogen?

a)

210.4mL

b)

514.3 mL

c)

700 mL

d)

1,711.1 mL

12.

Jacques Alexandre Charles performed an experiment in a balloon, hot water, and cold water. Which of the following statements is proposed in Charles’ Law?

a)

The Kelvin temperature and the volume of a gas are directly related at constant pressure.

b)

The pressure of a fixed amount of a gas is directly proportional to the absolute temperature (Kelvin).

c)

The volume of a given mass of gas held at constant temperature is inversely proportional to its pressure.

d)

The volume of a gas varies directly with the number of moles and absolute temperature and inversely proportional with pressure.

13.

Charles' Law deals with what quantities?

a)

pressure/temperature

b)

pressure/volume

c)

volume/temperature

d)

volume/temperature/pressure

14.
The following graph shows ____ relationship. 
a)
Direct
b)
Inverse
15.
Boyle's law :  The pressure and volume of a gas show a _____ relationship. 
a)
Inverse 
b)
Direct 
16.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm (make sure you use the correct R value).
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
17.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
18.
A sample of a gas has a volume of 852 mL at 298 K. What temperature is necessary for the gas to have a volume of 945 mL?
a)
Pt = P1 + P2 + P3 + ...
b)
P1V1 = P2V2
c)
V1/T1 = V2/T2
d)
P1V1/T1 = P2V2/T2
19.
The volume of a sample of a gas at 273 oC is 200 liters. If the volume is decreased to 100 liters at constant pressure, what will be the new temperature of the gas?
a)
0 K
b)
546 K
c)
273 K
d)
100 K
20.

If a hairspray can is heated, what can be expected of the pressure of the gas inside the can?

a)

The pressure will increase

b)

The pressure will decrease

c)

The pressure will remain constant

d)

The pressure will equalize

21.
Gases have...
a)
A definite shape and volume
b)
A definite shape but no definite volume
c)
No definite shape but a definite volume
d)
No definite shape or volume
22.
What is the variable for this number 22.4 L
a)
P
b)
T
c)
n
d)
V
23.
PV=nRT
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
24.
Which law helps us find the moles of gas in a sample?
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
25.
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
26.
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 
27.
Determine the Celsius temperature of 2.49 moles of gas contained in a 1.00-L vessel at a pressure of 143 kPa. 
a)
-266 degrees C
b)
-622 degrees C
c)
622 degrees C 
d)
266 degrees C
28.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 
a)
2
b)
3
c)
4
d)
6 
29.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
30.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
31.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
32.
Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
33.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
34.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
35.
How many grams of AgNO3 (MM = 169.87) are needed to prepare 0.125M solution in 250 mL of water? 
a)
.03g
b)
0.5g
c)
5.3g
d)
84.9g
36.
Which of the following has the most NaCl (MM = 58.44)?
a)
100 mL of a 1.8 M solution
b)
50 mL of a 4.1 M solution
c)
9.35 grams
d)
1 mole
37.
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
38.

Which of the following is the Dilution Formula?

a)

V1M1 = V2M2

b)

M = m/V

c)

V = mT

d)

PV = nRT

39.

Which of the following is the Dilution Formula?

a)

V1M1 = V2M2

b)

M = m/V

c)

V = mT

d)

PV = nRT

40.

A dilution is when

a)

solute is added to the volume of solution

b)

water is added to the volume of solution

c)

solute is removed from the volume of solution

d)

water is removed from the volume of solution

41.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

42.

What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250.0 mL?

a)

15.9 M

b)

0.636 M

c)

0.642 M

d)

1.59 M

43.
How many mL of 10.8M HCl 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
44.
What volume of 1.50 M 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
45.

If I have 340.0 mL of a 0.500 M NaBr solution, what will the concentration be if I add 560.0 mL more water to it? (Remember to use the total new volume)

a)

.188 M

b)

3.78 M

c)

.389 M

d)

1.76 M

46.

If I dilute 250 mL of 0.10 M lithium acetate solution to a volume of 750 mL, what will the concentration of this solution be?

a)

2 M

b)

0.02 M

c)

0.033 M

d)

0.08 M

47.
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
48.

125.0 mL of 2.00 M calcium hydroxide solution is diluted to a concentration of 1.50 M. How many mL of water was added to the original volume?

a)

167 mL

b)

42.0 mL

c)

93.8 mL

d)

0.0240 mL

49.

What is the percentage of OH– in Ca(OH)2?

a)

45.9%

b)

75%

c)

66.6%

d)

90.1%

50.

What is the mass of 3.35 moles of sulfur trioxide?

a)

335 g

b)

268 g

c)

245 g

d)

64 g

51.

How many moles are there in 425.0 g of sodium chloride?

a)

9.835 mol

b)

8.126 mol

c)

7.272 mol

d)

6.691 mol

52.

What is the mass of 5.55 moles of carbon monoxide?

a)

155 g

b)

143 g

c)

138 g

d)

122 g

53.

What is the gram formula mass of Silicon Tetrabromide?

a)

107.99 g/mol

b)

347.70 g/mol

c)

187.89 g/mol

d)

267.80 g/mol

54.

What is the molecular weight of iron (III) nitrate?

a)

145.847 g/mol

b)

117.854 g/mol

c)

241.8 g/mol

d)

85.854 g/mol

55.

The mass % of aluminum in aluminum sulfate is:

a)

12.93%

b)

45.70%

c)

7.89%

d)

35.94%

e)

15.77%

56.

The molar mass of potassium phosphate is:

a)

212.27 g

b)

251.37 g

c)

86.07 g

d)

173.17 g

e)

196.27 g

57.

The mass % of H in methane (CH4) is:

a)

75%

b)

92%

c)

25%

d)

4%

e)

6%

58.

In solving a mol conversion problem, you are asked to convert 25 grams of CO2 to total atoms. How many formulas would you use to do this conversions?

a)

One

b)

Two

c)

Three

d)

More that I can imagine. Perhaps to infinity and beyond.

59.

Find the percentage composition of Mg in Mg3(PO4)2.


a)

27.48% Mg

b)

43.11% Mg

c)

16.00% Mg

d)

12.63% Mg

60.
How many moles of NaCl are present in a solution with a molarity of 8.59M and 125 mL of solution?
a)
1.074 mol
b)
62.7 mol
c)
1.07 mol
d)
62.7 grams

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