1. No category

math review 2
Name: ____________________________________
Tuesday, May 20, 2008
1.
A sample of a gas has a volume of 2.0 liters at a pressure of 1.0 atmosphere. When the volume increases to 4.0 liters, at constant temperature, the
pressure will be
1. 1.0 atm
2. 2.0 atm
3. 0.50 atm
4. 0.25 atm
2.
The volume of a given mass of an ideal gas at constant pressure is
1. directly proportional to the Kelvin temperature
2. directly proportional to the Celsius temperature
3. inversely proportional to the Kelvin temperature
4. inversely proportional to the Celsius temperature
3.
If the pressure on a 3.0 liter sample of a gas is doubled at constant temperature, the new volume would be
1. 0.75 L
2. 1.5 L
3. 6.0 L
4. 9.0 L
4.
Figure 1
The diagram shows two flasks connected by a stop cock. Flask A contains helium gas. Flask B contains a vacuum. What final volume will the gas
occupy after the stopcock is open?
1. 100ml
2. 300ml
3. 400ml
4. 500ml
math review 2
5.
A sample of a gas occupies 6.00 liters at a temperature of 200 K. If the pressure remains constant and the temperature is raised to 600 K, the
volume of gas sample would be
1. 18.0 L
2. 2.00 L
3. 3.00 L
4. 12.0 L
6.
The temperature of 100 milliliters of a gas at 200.K is increased to 400.K, pressure remaining constant. The new volume of the gas will be
1. 50.0 ml
2. 100. ml
3. 200. ml
4. 400. ml
7.
Figure 2
The diagram represents four 500-milliliter flasks. Each contains the gas represented by the symbol. All gas samples are at STP. Each flask
contains the same number of
1. atoms, only
2. molecules, only
3. atoms and molecules
4. atoms, but different number of molecules
8.
At constant pressure which graph shows the correct relationship between the volume of a gas (v) and its absolute temperature (t)?
1.
2.
3.
4.
math review 2
9.
A sample of oxygen gas has a volume of 150. milliliters at 300 K. If the pressure of the sample is held constant and the temperature is raised to
600 K, the new volume of the sample will be
1. 75.0 mL
2. 150. mL
3. 300. mL
4. 600. mL
10.
If the pressure and Kelvin temperature of 2.00 moles of an ideal gas at STP are doubled, the resulting volume will be
1. 5.60 L
2. 11.2 L
3. 22.4 L
4. 44.8 L
11.
A gas has a volume of 2 liters at 323 K and 3 atmospheres. When its temperature is changed to 273 K and the pressure is changed to 1 atmosphere,
the new volume of the gas would be equal to
1.
2.
3.
4.
12.
A gas sample has a volume of 25.0 milliliters at a pressure of 1.00 atmosphere. If the volume increases to 50.0 milliliters and the temperature
remains constant, the new pressure will be
1. 1.00 atm
2. 2.00 atm
3. 0.250 atm
4. 0.500 atm
math review 2
13.
Figure 3
The table shows the temperature, pressure, and volume of five samples. Which sample contains the same number of molecules as sampleA?
1. E
2. B
3. C
4. D
14.
Which graph represents the relationship between volume and Kelvin temperature for an ideal gas at constant pressure?
3.
1.
4.
2.
15.
A closed container holds 3.0 moles of CO2 gas at STP. What is the total number of moles of Ne(g ) that can be placed in a container of the same
size at STP?
1. 1.0 mole
2. 1.5 moles
3. 3.0 moles
4. 0.0 moles
math review 2
16.
A 3.00-liter sample of gas is at 288 K and 1.00 atm. If the pressure of the gas is increased to 2.00 atm and its volume is decreased to 1.50 liters, the
Kelvin temperature of the sample will be
1. 144 K
2. 288 K
3. 432 K
4. 576 K
17.
A gas occupies a volume of 40.0 milliliters at 20°C. If the volume is increased to 80.0 milliliters at constant pressure, the resulting temperature
will be equal to
1.
2.
3.
4.
18.
Figure 4
The graph represents the heating curve of a substance that starts as a solid below its freezing point. What is the melting point of this substance?
1. 30°C
2. 55°C
3. 90°C
4. 120°C
math review 2
19.
The volume of a gas is 4.00 liters at 293 K and constant pressure. For the volume of the gas to become 3.00 liters, the Kelvin temperature must be
equal to
1.
2.
3.
4.
20.
Which graph best represents the pressure-volume relationship for an ideal gas at constant temperature?
1.
3.
2.
4.
21.
A gas occupies a volume of 444 mL at 273 K and 79.0 kPa. What is the final kelvin temperature when the volume of the gas is changed to 1880
mL and the pressure is changed to 38.7 kPa?
1. 31.5 K
2. 292 K
3. 566 K
4. 2360 K
math review 2
22.
A sample of helium gas has a volume of 900. milliliters and a pressure of 2.50 atm at 298 K. What is the new pressure when the temperature is
changed to 336 K and the volume is decreased to 450. milliliters?
1. 0.177 atm
2. 4.43 atm
3. 5.64 atm
4. 14.1 atm
23.
Cylinder A contains 22.0 grams of CO2(g) and cylinder B contains N2(g). The volumes, pressures, and temperatures of the
two gases are indicated under each cylinder.
Figure 5
Base your answer to the question on the information and diagrams.
The temperature of the CO2(g) is increased to 450. K and the volume of cylinderA remains constant. What is a correct numerical setup for
calculating the new pressure of the CO2(g) in cylinder A?
1.
2.
3.
4.
math review 2
24.
A sample of oxygen gas in one container has a volume of 20.0 milliliters at 297 K and 101.3 kPa. The entire sample is transferred to another
container where the temperature is 283 K and the pressure is 94.6 kPa. Which is a correct numerical setup for calculating the new volume of this
sample of oxygen gas?
1.
2.
3.
4.
25.
Base your answer to the question on the table below.
Figure 6
The volume of 1.00 mole of hydrogen bromide at STP is 22.4 liters. The gram-formula mass of hydrogen bromide is 80.9 grams per mole. What is
the density of hydrogen bromide at STP?
Answer:
g/L
math review 2
26.
Base your answer to the question on the information below.
Air bags are an important safety feature in modern automobiles. An air bag is inflated in milliseconds by the explosive
decomposition of NaN3(s). The decomposition reaction produces N2(g), as well as Na(s), according to the unbalanced equation
below.
NaN3(s)
Na(s) + N2(g)
Figure 7
When the air bag inflates, the nitrogen gas is at a pressure of 1.30 atmospheres, a temperature of 301 K, and has a volume of 40.0 liters. Calculate
the volume of the nitrogen gas at STP.
Answer:
L
27.
Base your answer to the question on the information below.
Archimedes (287-212 BC), a Greek inventor and mathematician, made several discoveries important to science today.
According to a legend, Hiero, the king of Syracuse, commanded Archimedes to find out if the royal crown was made of gold,
only. The king suspected that the crown consisted of a mixture of gold, tin, and copper.
Archimedes measured the mass of the crown and the total amount of water displaced by the crown when it was completely
submerged. He repeated the procedure using individual samples, one of gold, one of tin, and one of copper. Archimedes was
able to determine that the crown was not made entirely of gold without damaging it.
Figure 8
Determine the volume of a 75-gram sample of gold at STP.
Answer:
cm3
math review 2
28.
Base your answer to the question on the information below.
A rigid cylinder is fitted with a movable piston. The cylinder contains a sample of helium gas, He(g), which has an initial volume
of 125.0 milliliters and an initial pressure of 1.0 atmosphere, as shown below. The temperature of the helium gas sample is 20.0°C.
Figure 9
Express the initial volume of the helium gas sample, in liters.
Answer:
L
29.
[Refer to figure 9 in question 28]
The piston is pushed further into the cylinder. The temperature of the helium gas remains constant. Which is a correct numerical setup for
calculating the volume of the helium gas that is anticipated when the reading on the pressure gauge is 1.5 atmospheres?
1.
2.
3. (1.0)(125.0) = (1.50)(V2)
4. (1.50)(125.0) = (1.0)(V2)
math review 2
30.
At STP, which sample contains the same number of molecules as 11.2 liters of CO2(g) at STP?
1. 5.6 L of NO2(g)
3. 11.2 L of N2(g)
2. 7.5 L of H2(g)
4. 22.4 L of CO(g)
31.
The table below shows mass and volume data for four samples of substances at 298 K and 1 atmosphere.
Which two samples could consist of the same substance?
1. A and B
3. B and C
2. A and C
4. C and D
32.
What occurs when the temperature of 10.0 grams of water is changed from 15.5°C to 14.5°C?
1. The water absorbs 42 joules.
2. The water releases 42 joules.
3. The water absorbs 4200 joules.
4. The water releases 4200 joules.
33.
The strongest intermolecular forces of attraction exist in a liquid whose heat of vaporization is
1. 100 J/g
2. 200 J/g
3. 300 J/g
4. 400 J/g
math review 2
34.
Figure 10
The graph represents a solid heated at a uniform rate, starting at a temperature below its melting point. Once the solid has reached its melting
point, how many minutes are required to completely melt the solid?
1. 6 min
2. 2 min
3. 8 min
4. 4 min
35.
Figure 11
The graph represents a substance, X, in the form of a gas uniformly cooled from an initial temperature of 140°C. The time, in minutes, required to
cool gas X from point B to a liquid at its freezing point is
1. 2.5
2. 10.0
3. 12.5
4. 15.0
math review 2
36.
The temperature of 15 grams of water increased 3.0°C. How much heat was absorbed by the water?
1. 150J
2. 45J
3. 18.9J
4. 189J
37.
When 200 grams of water cools from 50.°C to 25°C, the total amount of heat energy released by the water is
1. 210J
2. 21000J
3. 42000J
4. 1500J
38.
How many joules of heat are needed to raise the temperature of a 4.0-gram sample of water 8.0°C?
1. 13334J
2. 168J
3. 134.4J
4. 1680J
39.
How many joules of heat are required to raise the temperature of 20 grams of water from 30°C to 40°C?
1. 134J
2. 168J
3. 420J
4. 840J
math review 2
40.
Figure 12
The graph was constructed by a student to show the relationship between temperature and time as heat was uniformly added to a solid below its
melting point. What is the total length of time that the solid phase was in equilibrium with the liquid phase?
1. 6 min
2. 10 min
3. 8 min
4. 4 min
41.
The heat of fusion of a compound is 333.6 joules per gram. What is the total number of joules of heat that must be absorbed by a 15.0-gram
sample to change the compound from solid to liquid at its melting point?
1. 1304J
2. 168J
3. 420J
4. 5004J
42.
The vapor pressure of a liquid is 0.92 atm at 60°C. The normal boiling point of the liquid could be
1. 35°C
2. 45°C
43.
3. 55°C
4. 65°C
math review 2
Figure 13
Which of the following is a correct numerical setup for calculating the number of joules of heat gained by the water?
1. q = (150.0 g) (4.18 J/g·°C) (3.1°C)
2. q = (100.0 g) (4.18 J/g·°C) (3.1°C)
3. q = (100.0 g) (334 J/g·°C) (26.2°C)
4. q = (150.0 g) (334J/g·°C) (26.2°C)
math review 2
44.
What is the total number of joules released when a 5.00-gram sample of water changes from liquid to solid at 0°C?
1. 334 J
2. 1670 J
3. 2260 J
4. 11 300 J
45.
What amount of heat is required to completely melt a 29.95-gram sample of H2O(s) at 0°C?
1. 334 J
3. 1.00 ×103 J
2. 2260 J
4. 1.00 ×104 J
46.
When 0.50 liter of a 12 M solution is diluted to 1.0 liters, the molarity of the new solution is
1. 6.0 M
2. 2.4 M
3. 12 M
4. 24 M
47.
What is the total number of grams of NaOH (formula mass = 40.) needed to make 1.0 liter of a 0.20 M solution?
1. 20. g
2. 2.0 g
3. 80. g
4. 8.0 g
48.
How many grams of NaNO3 would have to be added to 100. grams of water at 45°C to make a saturated solution of this salt?
1. 100.
2. 110.
3. 120.
4. 130.
49.
When 20. milliliters of 1.0 M HCL is diluted to a total volume of 60. milliliters, the concentration of the resulting solution is
1. 1.0 M
2. 0.50 M
3. 0.33 M
4. 0.25 M
math review 2
50.
How many liters of a 0.5 M sodium hydroxide solution would contain 2 moles of solute?
1. 1L
2. 2L
3. 3L
4. 4L
math review 2
Answer Key for math review 2
1. 3
2. 1
3. 2
4. 4
5. 1
6. 3
7. 2
8. 1
9. 3
10. 4
11. 3
12. 4
13. 2
14. 3
15. 3
16. 2
17. 3
18. 2
19. 1
20. 4
21. 3
22. 3
23. 2
24. 2
25. 3.61
26. 47.2
27. 3.9
28. 0.125
29. 3
30. 3
31. 2
32. 2
33. 4
34. 4
35. 3
36. 4
37. 2
38. 3
39. 4
40. 4
41. 4
42. 4
43. 2
44. 2
45. 4
46. 1
47. 4
48. 2
49. 3
50. 4