Gas Laws And Principles: Trivia Quiz!
There are different types of gasses in existence, and over the week, we have been able to learn so much more about them and their characteristics. Did you know that compound gasses contain a combination of different atoms? Do you think you have what it takes to answer the question below based on all we learned? Give it a shot and get to find out!
Questions and Answers
- 1.
TRUE or FALSE. According to Charles Law, if you have a balloon inside a car at noon during a hot summer day the balloon molecules inside will increase in pressure.
- A.
True
- B.
False
Correct Answer
B. FalseExplanation
According to Charles Law Pressure is Constant.Rate this question:
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- 2.
In a nitrogen gas occupies has a volume of 500ml at a pressure of 0.971atm.What volumewill the gas occupy at a pressure of 1.50 atm, assuming the temperature remains constant?
- A.
342mL
- B.
424mL
- C.
324mL
- D.
442mL
- E.
242mL
Correct Answer
C. 324mLExplanation
According to Boyle's Law, the volume of a gas is inversely proportional to its pressure when the temperature remains constant. Therefore, we can use the formula V1P1 = V2P2 to solve this problem. Given that V1 = 500 mL, P1 = 0.971 atm, and P2 = 1.50 atm, we can substitute these values into the formula to find V2. Solving for V2, we get V2 = (V1P1) / P2 = (500 mL * 0.971 atm) / 1.50 atm = 324 mL. Therefore, the gas will occupy a volume of 324 mL at a pressure of 1.50 atm.Rate this question:
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- 3.
Not all Gas Law problems have Kelvin (K) as the unit of temperature. They can be expressed in Celsius (°C)and Fahrenheit(°F). So convert 123°C to K.
- A.
396K
- B.
486K
- C.
369K
- D.
458K
- E.
693K
Correct Answer
A. 396KExplanation
Gas law problems can be solved using different temperature units such as Celsius and Fahrenheit. In this question, the temperature is given in Celsius (123°C) and needs to be converted to Kelvin (K). To convert Celsius to Kelvin, we add 273 to the Celsius temperature. Therefore, 123°C + 273 = 396K.Rate this question:
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- 4.
Gas pressure is caused by
- A.
Gas molecules heating up
- B.
Gas molecules reacting with other gas molecules
- C.
Gas molecules hitting the walls of a container
- D.
Gas molecules hitting other gas molecules
Correct Answer
C. Gas molecules hitting the walls of a containerExplanation
Gas pressure is caused by gas molecules hitting the walls of a container. When gas molecules move around in a container, they collide with the walls, exerting a force on them. This force creates pressure within the container. The more frequent and energetic the collisions, the higher the gas pressure. The other options, such as gas molecules heating up, reacting with other gas molecules, or hitting other gas molecules, may affect the behavior of the gas but do not directly cause gas pressure.Rate this question:
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- 5.
At a pressure of 5.0 atmospheres, a sample of gas occupies 40. liters. What volume will the same sample occupy at 1.0 atmosphere?
- A.
0.0050 L
- B.
0.13 L
- C.
200 L
- D.
8.0 L
Correct Answer
C. 200 LExplanation
According to Boyle's Law, the volume of a gas is inversely proportional to its pressure, assuming the temperature and amount of gas remain constant. Therefore, if the pressure decreases from 5.0 atmospheres to 1.0 atmosphere, the volume of the gas will increase proportionally. Since the initial volume is 40 liters, the final volume can be calculated by multiplying the initial volume by the ratio of the initial pressure to the final pressure: 40 L * (5.0 atm / 1.0 atm) = 200 L.Rate this question:
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- 6.
As the volume of confined gad decreases at constant temperature, the pressure exerted by the gas ______.
- A.
Decreases
- B.
Increases
- C.
Stay the same
- D.
Fluctuates
Correct Answer
B. IncreasesExplanation
As the volume of confined gas decreases at constant temperature, the pressure exerted by the gas increases. This is because according to Boyle's Law, the pressure of a gas is inversely proportional to its volume when temperature is constant. Therefore, as the volume decreases, the gas particles become more crowded, leading to more frequent collisions with the walls of the container, resulting in an increase in pressure.Rate this question:
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- 7.
A sample of argon has a volume of 0.43 mL at 299K. At what temperature in degrees Celsius will it have a volume of 1 mL.
- A.
695°C
- B.
422°C
- C.
428°C
- D.
694°C
Correct Answer
B. 422°CExplanation
At a constant pressure, the volume of a gas is directly proportional to its temperature in Kelvin according to Charles's Law. Therefore, to find the temperature at which the volume of argon becomes 1 mL, we can use the equation V1/T1 = V2/T2. Plugging in the given values, we have 0.43 mL/299K = 1 mL/T2. Solving for T2 gives us T2 = (1 mL * 299K) / 0.43 mL = 695.35K. Converting this temperature to degrees Celsius, we get 695°C. Therefore, the correct answer is 695°C.Rate this question:
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- 8.
Each of these flasks contains the same number of molecules. In which container is the pressure highest?
- A.
Flask 1
- B.
Flask 2
- C.
Flask 3
- D.
Flask 4
- E.
Flask 5
Correct Answer
A. Flask 1Explanation
As the volume decrease the pressure increases because there are more collisions per unit of surface area within the container.Rate this question:
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- 9.
TRUE or FALSE: A good example of Charles Law is when a piece of metal expands in the heat
- A.
True
- B.
False
Correct Answer
B. FalseExplanation
Gas laws are not applicable to SOLIDSRate this question:
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- 10.
Assuming that the temperature remains constant. How can you increase the pressure of a gas?
- A.
Increase the container volume
- B.
Add more molecules of the gas
- C.
Decreases the container volume
- D.
None of the above
Correct Answer
D. None of the aboveExplanation
The pressure of a gas can be increased by adding more molecules of the gas or by decreasing the container volume. However, in this question, it is stated that the temperature remains constant. Therefore, increasing the container volume or adding more molecules of the gas will not affect the pressure, as these factors are only relevant when the temperature is not constant.Rate this question:
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- 11.
In a closed container at 1.0 atmosphere, the temperature of a sample of gas is raised from 300 K to 400 K. What will be the final pressure of the gas?
- A.
0.010 atm
- B.
0 atm
- C.
100 atm
- D.
1.3 atm
Correct Answer
D. 1.3 atmExplanation
When the temperature of a gas in a closed container is increased, the gas molecules gain more kinetic energy and move faster. This increased motion results in more frequent and forceful collisions with the container walls, causing an increase in pressure. According to Charles's Law, which states that at constant pressure, the volume of a gas is directly proportional to its temperature, the increase in temperature will cause the gas to expand and therefore increase the pressure. Therefore, the final pressure of the gas will be higher than the initial pressure of 1.0 atm, resulting in a final pressure of 1.3 atm.Rate this question:
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- 12.
At constant pressure and 25 °C a sample of gas occupies 4.5 liters. At what temperature will the gas occupy 9.0 liters?
- A.
596K
- B.
50K
- C.
50°C
- D.
596°C
Correct Answer
C. 50°CExplanation
The answer is 50°C because according to Charles's Law, the volume of a gas is directly proportional to its temperature when pressure is constant. In this case, the initial volume of the gas is 4.5 liters at 25°C. If the volume doubles to 9.0 liters, the temperature must also double. Therefore, the final temperature is 50°C.Rate this question:
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- 13.
TRUE OR FALSE. You drove continuously from Laguna to Manila and you observed that the pressure in your tires increased. This is because of the increased temperature outside the tire caused by friction.
- A.
True
- B.
False
Correct Answer
B. FalseExplanation
The statement is false because the pressure in the tires actually decreases as the temperature increases. This is because the air inside the tires expands when heated, causing the pressure to decrease. So, if the pressure in the tires increased during the drive, it would not be due to the increased temperature caused by friction.Rate this question:
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- 14.
Each of these flasks contains the same number of gas molecules. In which would the pressure be lowest?
- A.
Flask 1
- B.
Flask 2
- C.
Flask 3
- D.
Flask 4
Correct Answer
A. Flask 1Explanation
As the temperature decreases, molecules move more slowly and collide with the walls of the container less often.Rate this question:
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- 15.
Neon gas has a volume of 2,000ml with an atm of 1.8 however the pressure decreased to 1.3atm what is now the volume of the neon gas?
- A.
2, 795mL
- B.
2,759mL
- C.
3,795mL
- D.
3,759mL
Correct Answer
B. 2,759mLExplanation
When the pressure of a gas decreases, its volume increases, assuming all other factors remain constant. In this case, the initial volume of the neon gas is given as 2,000 mL and the initial pressure is 1.8 atm. When the pressure decreases to 1.3 atm, the volume of the gas would increase. Therefore, the correct answer is 2,759 mL, which is a larger volume than the initial 2,000 mL.Rate this question:
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- 16.
Each of these flasks is the same size and at the same temperature. Which one contains the most molecules?
- A.
Flask 1
- B.
Flask 2
- C.
Flask 3
- D.
Flask 4
Correct Answer
D. Flask 4Explanation
The highest pressure indicates the greatest number of collisions with the wall of the container, and therefore the most molecules.Rate this question:
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- 17.
When a supply of hydrogen gas is held in a 4 liter container at 320 K it exerts a pressure of 800 torr. The supply is moved to a 2 liter container, and cooled to 160 K. What is the new pressure of the confined gas?
- A.
800 torr
- B.
1600 torr
- C.
200 torr
- D.
400 torr
Correct Answer
A. 800 torrExplanation
According to the ideal gas law, the pressure of a gas is directly proportional to its temperature and inversely proportional to its volume. In this case, the volume is halved (from 4 liters to 2 liters) and the temperature is halved (from 320 K to 160 K). Since the volume is halved, the pressure will double. Since the temperature is halved, the pressure will also halve. Therefore, the new pressure of the gas will be the same as the original pressure, which is 800 torr.Rate this question:
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- 18.
Which Gas Law is involved when a balloon pops after being sat on?
- A.
Charles Law
- B.
Boyle's Law
- C.
Law of Pressure Gradient
- D.
None of the Above
Correct Answer
B. Boyle's LawExplanation
According to Boyles Law “at constant temperature, increases in pressure is directly proportional to increase in volume.Rate this question:
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- 19.
A small sample of helium gas occupies 6 mL at a temperature of 250 K. At what temperature does the volume expand to 9 mL?
- A.
125K
- B.
375K
- C.
500K
- D.
2250K
Correct Answer
B. 375KExplanation
When a gas expands, its volume increases. According to Charles's Law, the volume of a gas is directly proportional to its temperature, assuming constant pressure. In this question, the initial volume is 6 mL at a temperature of 250 K, and the final volume is 9 mL. Since the volume is increasing, the temperature must also increase. The correct answer is 375K because it is the only option that represents a higher temperature than the initial temperature, leading to the expansion of the gas.Rate this question:
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- 20.
Organize the following gases in order of their rates of difusion, from slowest to fastest oxygen, O2 ammonia, NH3 hydrogen, H2 carbon dioxide, CO2
- A.
Hydrogen, oxygen, carbon dioxide, ammonia
- B.
Oxygen, hydrogen, carbon dioxide, ammonia
- C.
Hydrogen, ammonia, oxygen, carbon dioxide
- D.
Hydrogen, oxygen, ammonia, carbon dioxide
- E.
Carbon dioxide, oxygen, ammonia, hydrogen
Correct Answer
E. Carbon dioxide, oxygen, ammonia, hydrogenExplanation
The given answer is correct because it correctly organizes the gases in order of their rates of diffusion. Carbon dioxide has the slowest rate of diffusion, followed by oxygen, ammonia, and hydrogen, which has the fastest rate of diffusion.Rate this question:
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Test Your Knowledge About Isotopes of Hydrogen Quiz
Test Your Knowledge About Isotopes of Hydrogen Quiz
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