Gas Laws Quiz: Boyle's And Charles' Law

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Matt Balanda, BS (Aerospace Engineering) |
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Matt Balanda, a Calvary Chapel Christian School leader with a Bachelor's in Aerospace Engineering and Mathematics, transitioned from Aerospace Engineering to Education with a Master's from California Baptist University. As the High School Vice-Principal and Physics teacher, he nurtures students' love of learning and faith, creating an enriching and transformational educational experience.
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1. What is the final pressure in a balloon when the volume is changed from 1.5  L to a volume of 2.5L at constant temperature? (Initial pressure is 1.1 atm).

Explanation

To find the final pressure (Pf) when the volume changes at constant temperature, you can use Boyle's Law, which states that the product of pressure and volume is constant for a given amount of gas at constant temperature.



The formula for Boyle's Law is given by:



P1 . V1 = P2. V2

where:

- ( P1) is the initial pressure,

- (V1)  is the initial volume,

- ( P2) is the final pressure,

- ( V2) is the final volume.



Given:

- (P1 = 1.1 ) atm (initial pressure),

- ( V1 = 1.5 ) L (initial volume),

- ( V2= 2.5 ) L (final volume).



Plug in the values into Boyle's Law:



[ 1.1. 1.5] L = P2. 2.5 L



Now, solve for P2



P2 = 1.1 atm . 1.5L/ 2.5L

P2 ≈ 0.66 atm



Therefore, the final pressure in the balloon when the volume changes from 1.5 L to 2.5 L at constant temperature is approximately 0.66 atm.

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About This Quiz
Gas Laws Quiz: Boyles And Charles Law - Quiz


Welcome to the Gas Laws: Boyle's and Charles' Law Quiz, where you'll delve into the fascinating principles governing the behavior of gasses. Boyle's Law and Charles' Law are... see morefoundational concepts in the study of gas physics. As you navigate through this quiz, you'll be challenged to apply these laws in various scenarios and explore their implications on gas behavior. This quiz aims to assess your ability to apply these fundamental gas laws to real-world situations, providing a comprehensive understanding of how gasses respond to changes in pressure, volume, and temperature. Best of luck as you navigate the intricacies of Boyle's and Charles' Laws!
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2. A balloon occupies 3.2 L at 37oC. How much volume will it occupy at 42oC?

Explanation

Using the formula,

V1/T1=V2/T2 and substituting the values of V1,T1 and T2 and solving the equation we get,

Given:

V1​=3.2L at T1​= 37°C =310.15K

T2=42°C =315.15 K

3.2L/315.15K=V2/310.15K

Therefore 

V2=3.2L x 310.15K/315.15K

V2​≈3.25L

Therefore, the balloon will occupy approximately 3.25 L at 42°C.

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3. If the air inside a balloon is heated, the volume will:

Explanation

If the air inside a balloon is heated while the pressure remains constant, the volume of the balloon will generally increase. This behavior follows Charles's Law, which states that the volume of a gas is directly proportional to its temperature at constant pressure.

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4. What is the final pressure in a vessel when the volume is changed from 1.3  L to a volume of 1.55 L at constant temperature? (Initial pressure is 1.5 atm).

Explanation

The formula for Boyle's Law is given by:



P1 . V1 = P2. V2

where:

- ( P1) is the initial pressure,

- (V1)  is the initial volume,

- ( P2) is the final pressure,

- ( V2) is the final volume.



Given:

- (P1 = 1.5 ) atm (initial pressure),

- ( V1 = 1.3 ) L (initial volume),

- ( V2= 1.55 ) L (final volume).



Plug in the values into Boyle's Law:



[ 1.5. 1.3] L = P2. 1.55 L



Now, solve for P2



P2 = 1.5 atm .  1.3L/ 1.55L

P2 ≈1.26atm

Therefore, the final pressure in the vessel when the volume changes from 1.3 L to 1.55 L at constant temperature is approximately 1.26 atm.

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5. A gas occupies a balloon with a volume 2.0 L at 33oC. How much volume will it occupy at 37oC, if pressure remains constant?

Explanation

Using the formula,

V1/T1=V2/T2 and substituting the values of V1,T1 and T2 and solving the equation we get,

Given:

V1​=2.0L at T1​= 33°C =306.15K

T2=37°C =310.15 K

2.0L/306.15K=V2/310.15K

Therefore 

V2=2.0L x 310.15K/306.15K

V2​≈2.026L

Therefore, the balloon will occupy approximately 2.026 L at 37°C.

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6. A gas expands from a volume 2.0 L at 36oC to a volume of 2.5 L. What is the final temperature (in Kelvin) if the pressure is constant?

Explanation

Using the formula,

V1/T1=V2/T2 and substituting the values of V1,T1 and V2 and solving the equation we get,

Given:

V1​=2.0L at T1​= 36°C =309.15K

V2=2.5L

2.0L/309.15K=2.5L/T2

Therefore 

T2=2.5L x 309.15K / 2.0 L

T2​≈ 386.43 K

Therefore, the final temperature is approximately 386.43 K when the gas expands from a volume of 2.0 L at 36°C to a volume of 2.5 L, assuming the pressure remains constant.

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7. A balloon occupies a volume of 2.0 L at 40oC. How much volume will it occupy at 30oC?

Explanation

Using the formula,

V1/T1=V2/T2 and substituting the values of V1,T1 and T2 and solving the equation we get,

Given:

V1​=2.0L at T1​= 40°C =313.15K

T2=30°C =303.15 K

2.0L/313.15K=V2/313.15K

Therefore 

V2=2.0L x 303.15K/313.15K

V2​≈1.94L

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8. The kinetic theory of gasses, which of the following is important for an ideal gas:

Explanation

The correct answer is that there is no attraction or repulsion between the gas molecules, whereas there IS attraction between molecules of liquids or solids. This is important for an ideal gas because it assumes that the gas molecules do not interact with each other, except during collisions. This allows for simplifications in the mathematical models used to describe the behavior of ideal gasses. In contrast, liquids and solids have intermolecular forces that result in attractions between their molecules, leading to different behaviors and properties.

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9. Which of the following describes the relationship between P and V?            

Explanation

The relationship between P and V is described as inversely proportional. This means that as one variable (P) increases, the other variable (V) decreases, and vice versa. In other words, there is a negative correlation between P and V, where an increase in one variable corresponds to a decrease in the other variable.

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10. Gas in a balloon occupies 3.3  L. What volume will it occupy if the pressure is changed from 100 kPa to 90  kPa (at constant temperature of 310 K (about room temperature)?

Explanation

The formula for Boyle's Law is given by:



P1 . V1 = P2. V2

where:

- ( P1) is the initial pressure,

- (V1)  is the initial volume,

- ( P2) is the final pressure,

- ( V2) is the final volume.



Given:

- P1 = 100 kPa (initial pressure),

- V1 = 3.3 L (initial volume),

- P2 = 90 kPa (final volume)

T = 310K (Constant Temperature)



Plug in the values into Boyle's Law to find V2:

V2 = P1 . V1 / P2

Now, solve for V2

V2 =100 kPa .  3.3L/ 90kPa

V2 ≈ 3.67L



Therefore, the volume the gas will occupy when the pressure is changed from 100 kPa to 90 kPa at constant temperature is approximately 3.67 L.

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Matt Balanda |BS (Aerospace Engineering) |
Science Teacher
Matt Balanda, a Calvary Chapel Christian School leader with a Bachelor's in Aerospace Engineering and Mathematics, transitioned from Aerospace Engineering to Education with a Master's from California Baptist University. As the High School Vice-Principal and Physics teacher, he nurtures students' love of learning and faith, creating an enriching and transformational educational experience.

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What is the final pressure in a balloon when the volume is...
A balloon occupies 3.2 L at 37oC. How much volume will it occupy at...
If the air inside a balloon is heated, the volume will:
What is the final pressure in a vessel when the volume is...
A gas occupies a balloon with a volume 2.0 L at 33oC. How...
A gas expands from a volume 2.0 L at 36oC to a volume of 2.5...
A balloon occupies a volume of 2.0 L at 40oC. How much volume will it...
The kinetic theory of gasses, which of the following is important for...
Which of the following describes the relationship between P and V? ...
Gas in a balloon occupies 3.3  L. What volume will it occupy...
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