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High School Chemistry : Using Boyle's Law

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Example Questions

Example Question #11 : Gases And Gas Laws

An ideal gas exerts a pressure of $\small 3atm$ in a $\small 3L$ container. The container is at a temperature of $\small 298K$ .

What will be the final pressure if the volume of the container changes to $\small 2L$ ?

Possible Answers:

2 atm

4atm

4.5atm

3.5atm

Correct answer:

4.5atm

Explanation:

Since the volume of the gas is the only variable that has changed, we can use Boyle's law in order to find the final pressure. Since pressure and volume are on the same side of the ideal gas law, they are inversely proportional to one another. In other words, as one increases, the other will decrease, and vice versa.

Boyle's law can be written as follows:

$P_{1}V_{1} = P_{2}V_{2}$

Use the given volumes and the initial pressure to solve for the final pressure.

$(3atm)(3L) = (2L)P_{2}$

$P_{2} = 4.5atm$

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Example Question #1 : Using Boyle's Law

What law is the following formula?

$P_{1}V_{1}= P_{2}V_{2}$

Possible Answers:

Charles's law

Boyle's law

Combined gas law

Ideal gas law

Gay-Lussac's law

Correct answer:

Boyle's law

Explanation:

Boyle's law relates the pressure and volume of a system, which are inversely proportional to one another. When the parameters of a system change, Boyle's law helps us anticipate the effect the changes have on pressure and volume.

P_1V_1=P_2V_2

Charles's law relates temperature and volume: $\frac{V_1}{T_1}=\frac{V_2}{T_2}$

Gay-Lussac's law relates temperature and pressure: $\frac{P_1}{T_1}=\frac{P_2}{T_2}$

The combined gas law takes Boyle's, Charles's, and Gay-Lussac's law and combines it into one law: $\frac{P_{1}V_{1}}{T_{1}}=\frac{P_{2} V_{2}}{T_{2}}$

The ideal gas law relates temperature, pressure, volume, and moles in coordination with the ideal gas constant: PV=nRT

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Example Question #13 : Gases And Gas Laws

A helium balloon has a volume of 735mL when it is at ground level. The balloon is transported to an elevation of 5km , where the pressure is only 0.8atm . At this altitude the gas occupies a volume of 1286mL . Assuming the temperature has remained the same, what was the ground level pressure?

Possible Answers:

1.4atm

1.2atm

0.7atm

1.0atm

Correct answer:

1.4atm

Explanation:

To solve this question we will need to use Boyle's law:

P_1V_2=P_2V_2

We are given the final pressure and volume, along with the initial volume. Using these values, we can calculate the initial pressure.

P_1(735mL)=(0.8atm)(1286mL)

$P_1=\frac{(0.8atm)(1286mL)}{735mL}$

P_1=1.4atm

Note that the pressure at sea level is equal to 1.0atm . A pressure greater than 1.0atm simply indicates that the ground level is below sea level at this point.

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Example Question #14 : Gases And Gas Laws

The graph depicted here represents which of the gas laws?

Boyle_s_law_graph

Possible Answers:

Hund's law

Charles's law

Gay-Lussac's law

Boyle's law

Correct answer:

Boyle's law

Explanation:

The graph shows that there is an inverse relationship between the volume and pressure of a gas, when kept at a constant temperature. This was described by Robert Boyle and can be represented mathematically as Boyle's law:

P_1V_1=P_2V_2

Gay-Lussac's law shows the relationship between pressure and temperature. Charles's law shows the relationship between volume and temperature. Hund's rule (Hund's law) is not related to gases, and states that electron orbitals of an element will be filled with single electrons before any electrons will form pairs within a single orbital.

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Example Question #1 : Using Boyle's Law

A sample of oxygen gas has a volume of 225mL when its pressure is 1.12atm . What will the volume of the gas be at a pressure of 0.98atm if the temperature remains constant?

Possible Answers:

220mL

250mL

257mL

316mL

Correct answer:

257mL

Explanation:

To solve this question we will need to use Boyle's law:

P_1V_2=P_2V_2

We are given the initial pressure and volume, along with the final pressure. Using these values, we can calculate the final volume.

(1.12atm)(225mL)=(0.98atm)V_2

$V_2=\frac{(1.12atm)(225mL)}{0.98atm}$

V_2=257mL

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Example Question #1 : Using Boyle's Law

A gas is initially in a 5L piston with a pressure of 1atm.

If pressure changes to 3.5atm by moving the piston down, what is new volume?

Possible Answers:

1.75 L

1.43 L

2.03 L

2.7 L

1. 31 L

Correct answer:

1.43 L

Explanation:

Use Boyle's Law:

P_1*V_1 = P_2*V_2

Plug in known values and solve for final volume.

5L+1atm=3.5atm*V_2

V_2=1.43L

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Example Question #1 : Using Boyle's Law

A balloon of volume .666L at 1.03atm is placed in a pressure chamber where the pressure becomes 5.68atm , determine the new volume.

Possible Answers:

1.27L

.121L

.236L

.467L

.033L

Correct answer:

.121L

Explanation:

Use Boyle's law and plug in appropriate parameters:

P_1V_1=P_2V_2

.666L*1.03atm=5.68atm*V_2

$\frac{.666L*1.03atm}{5.68L}=V_2$

.121L=V_2

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Example Question #1 : Using Boyle's Law

A gas in a $30.0\, mL$ container is at $1.05\, atm$ is compressed to a volume of $15.0\, mL$ . What is the new pressure of the container?

Possible Answers:

$P_{2}=0.525\, atm$

$P_{2}=472.5\, atm$

$P_{2}=2.10\, atm$

$P_{2}=1.05\, atm$

Correct answer:

$P_{2}=2.10\, atm$

Explanation:

Boyle's Law is:

$P_{1} V_{1}=P_{2} V_{2}$

The initial volume ( $V_{1}$ ) and pressure ( $P_{1}$ ) of the gas is given. The volume changes to a new volume ( $V_{2}$ ). Our goal is to find the new pressure ( $P_{2}$ ). Solving for the new pressure gives:

$\frac{P_{1} V_{1}}{V_{2}}=\frac{P_{2} V_{2}}{V_{2}}\rightarrow P_{2}=\frac{P_{1} V_{1}}{V_{2}}$

$P_{2}=\frac{(1.05\, atm)(30\, mL)}{15\, mL}=2.10\, atm$

Notice the answer has 3 significant figures.

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High School Chemistry : Using Boyle's Law

Study concepts, example questions & explanations for High School Chemistry

All High School Chemistry Resources

Example Questions

Example Question #11 : Gases And Gas Laws

Example Question #1 : Using Boyle's Law

Example Question #13 : Gases And Gas Laws

Example Question #14 : Gases And Gas Laws

Example Question #1 : Using Boyle's Law

Example Question #1 : Using Boyle's Law

Example Question #1 : Using Boyle's Law

Example Question #1 : Using Boyle's Law

All High School Chemistry Resources

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