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×02nd Nov 2019 @ 5 min read

Write a brief answer to the following questions. If you think it is necessary, you may use illustrations to support your answer.

Explain Boyle's law with its equation?

Is Boyle's law universally true? If not, what are its limitations?

Give some real-life examples of Boyle's law?

Explain *PV* curve?

Can Boyle's law be experimentally proven? If yes, write in a few words how would you?

What happens when the pressure of a gas is double at a constant temperature?

Solve the following problems.

Methane gas is compressed isothermally from 1.00 atm to 1.75 atm. The initial volume is 20 L. Find the final volume of the gas?

Nitrogen gas expands isothermally from 10 cm^{3} to 25 cm^{3}. The initial pressure is 2.0 × 10^{5} Pa. Determine the final pressure of nitrogen?

The pressure of a gas changes from 2.50 bar to 0.80 bar. The final volume is 100 mL. Find the initial volume?

Steam is stored inside an industrial vessel of 4.2 m^{3}. After compression, the volume of steam reduces to 1.1 m^{3}. Assume the temperature to be constant. Find the initial pressure if the final pressure is 4 bar?

The pressure of oxygen gas at 25 °C is 500 kPa. If the volume of the gas is double, what will be its new pressure?

A balloon of hydrogen is subjected to vacuum. The initial pressure and volume of hydrogen is 0.95 atm and 0.55 L. Calculate the final pressure if the final volume is 1.22 L?

A gas occupies 22.2 L at a pressure of 760 mmHg. Find the new volume if the pressure is reduced to 120 mmHg?

A student collects an experimental gas of a volume of 730 mL at 101 kPa. What will be the volume at 202 kPa?

An astronaut releases a compressed gas into space. The initial volume is 20 L. What is the final volume?

A balloon is transported from London to Paris. The volume and pressure of the balloon in London is 2.2 L and 0.95 atm and the pressure in Paris is 1.2 atm. Assuming the temperature to be constant, find the volume of the balloon in Paris?

An experiment is performed on a gas to studies its behaviour. The pressure-volume data at constant temperature for a fixed amount of the gas is recorded. The data is as follows:

Pressure (atm) | 0.9 | 1.2 | 1.3 | 1.5 | 1.8 | 1.9 | 2.1 |
---|---|---|---|---|---|---|---|

Volume (L) | 24.9 | 18.6 | 17.1 | 15.0 | 12.1 | 11.5 | 10.2 |

Find whether the gas obeys Boyle's law by plotting the graph of pressure vs volume and pressure vs inverse volume?

Propane gas is stored in an industrial vessel of 3.2 m^{3}. A pressure gauge attached to the vessel shows a reading of 500.5 kPa. The atmospheric pressure is 101.3 kPa. Later the gas is transfer to a reactor of 4.0 m^{3}. What is the pressure reading of a pressure gauge attached to the reactor if the temperature remains the same?

Hint: Gauge pressure = Absolute pressure − Atmospheric pressure

Find the missing quantity from the following data.

*P*_{1}= 1.61 atm,*V*_{1}= 11.3 m^{3},*P*_{2}= 2.13 atm,*V*_{2}= ?*P*_{1}= 0.75 bar,*V*_{1}= 1.0 L,*P*_{2}= ?,*V*_{2}= 2.0 L*P*_{1}= 3.119 × 10^{5}Pa,*V*_{1}= ?,*P*_{2}= 5.152 × 10^{5}Pa,*V*_{2}= 100.9 cm^{3}*P*_{1}= ?,*V*_{1}= 8.8 L,*P*_{2}= 5.33 atm,*V*_{2}= 15.4 L

- Follow the link.
- Check the limitations section of the article link.
- Follow the link.
- Follow the link.
- Follow the link.
- When the pressure of a gas is double the volume is reduced by half as per Boyle's law.

- Ans: 11 L
- Ans: 0.80 × 10
^{5}Pa - Ans: 32 mL
- Ans: 1 bar
- Ans: The pressure is reduced by half.
- Ans: 0.43 atm
- Ans: 140 L
- Ans: 365 L
- Ans: ∞. The pressure in space is zero so the volume will expand infinitely.
- Ans: 1.7 L
- The graph of pressure vs volume is hyperbolic as expected. And the graph of pressure vs inverse volume is a straight line with positive slope passing through the origin. Hence, the gas obeys Boyle's law.
- Ans: 380.1 kPa
- Ans: 8.54 m
^{3} - Ans: 0.38 bar
- Ans: 166.7 cm
^{3} - Ans: 9.3 atm

- Ans: 8.54 m

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Thanks for your response!

Naomi

20th Oct 2020

20th Oct 2020

Wow it's awesome!!

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