Question 1

What unit of temperature is used in gas law calculations?

Accepted Answer

Gas law calculations require the use of the absolute temperature scale, which is measured in Kelvin. Degrees Celsius and Fahrenheit are both relative temperature scales and cannot be used in gas law calculations without conversion to Kelvin.

Question 2

An autoclave is used to sterilize surgical equipment because

Accepted Answer

An autoclave increases the pressure, allowing water to boil at temperatures above 100 °C, which is necessary for effective sterilization.

Question 3

The temperature of a 500. mL sample of gas increases from 150. K to 350. K. What is the final volume of the sample of gas, if the pressure and moles in the container is kept constant?

Accepted Answer

According to Charles's Law (V1/T1 = V2/T2), if the pressure and moles are constant, the volume of a gas is directly proportional to its temperature in Kelvin. V2 = V1 * (T2/T1) = 500 mL * (350 K / 150 K) = 1166.67 mL, which rounds to 1170 mL.

Question 4

Vapor pressure can be described as

Accepted Answer

Vapor pressure is the pressure exerted by a gas above the surface of its liquid. It is the result of the molecules in the liquid being in constant motion and some of them escaping into the gas phase. The vapor pressure increases with temperature and is a measure of the tendency of the liquid to evaporate.

Question 5

When the combined gas law is rearranged to solve for V₂, the following is the correct expression: V₂ =

Accepted Answer

The combined gas law is (P1V1/T1) = (P2V2/T2). Solving for V2 gives V2 = (P1V1T2)/(P2T1).

Question 6

A balloon is filled with helium gas. For the question(s) that follow, select the letter of the balloon diagram that corresponds to the given change in conditions. 
-The balloon is put into a chamber whose pressure is less than the atmospheric pressure and at atmospheric temperature.

Accepted Answer

The answer of A balloon is filled with helium gas....

Question 7

The boiling point of water at sea level is 100 °C. At higher altitudes, the boiling point of water will be

Accepted Answer

The boiling point of water is dependent on atmospheric pressure, and as altitude increases, atmospheric pressure decreases. Therefore, the boiling point of water at higher altitudes will be lower than 100°C.

Question 8

A balloon is filled with helium gas. For the question(s) that follow, select the letter of the balloon diagram that corresponds to the given change in conditions. 
-The temperature is changed from 50 °C to -150 °C at constant pressure.

Accepted Answer

The answer of A balloon is filled with helium gas....

Question 9

In Gay-Lussac's Law, the pressure of a gas increases due to an increase in temperature because

Accepted Answer

According to Gay-Lussac's Law, if the temperature of a gas increases, the pressure will also increase, assuming that the volume of the gas and the amount of gas present remain constant. This is because an increase in temperature causes the gas molecules to move faster and strike the walls of the container more often, resulting in a higher pressure.

Question 10

A sample of helium gas at 27.0 °C and 3.60 atm pressure is cooled in the same container to a temperature of -73.0 °C. What is the new pressure?

Accepted Answer

Using the ideal gas law and assuming constant volume, the pressure is directly proportional to temperature in Kelvin. Convert temperatures to Kelvin (27°C = 300K, -73°C = 200K) and use P1/T1 = P2/T2 to find the new pressure: (3.60 atm / 300K) = (P2 / 200K), solving gives P2 = 2.40 atm.

Question 11

A gas sample in a closed, expandable container of initial volume 5.00 L was allowed to warm from 25 °C to 35 °C, at constant moles and pressure. What was its new volume?

Accepted Answer

According to Charles's Law, at constant pressure, the volume of a gas is directly proportional to its temperature (in Kelvin). Therefore, if the temperature increases from 25 °C (298 K) to 35 °C (308 K), the volume should increase in the same ratio. The new volume can be calculated as:
new volume = (initial volume) x (new temperature / initial temperature) = 5.00 L x (308 K / 298 K) = 5.17 L
Thus, choice B is the correct answer.

Question 12

A sample of argon gas at 300. °C and 50.0 atm pressure is cooled in the same container to a temperature of 0.00 °C. What is the new pressure?

Accepted Answer

The answer of A sample of argon gas at 300....

Question 13

As the temperature of a gas increases, the density of the gas will

Accepted Answer

As the temperature of a gas increases, the kinetic energy of the gas particles increases causing them to move faster and spread out more. This results in a decrease in density.

Question 14

The temperature of a 350. mL sample of gas increases from 27 °C . to 227 °C . What is the final volume of the sample of gas, if the pressure and moles in the container is kept constant?

Accepted Answer

Using Charles's Law (V1/T1 = V2/T2), convert temperatures to Kelvin (T1 = 300 K, T2 = 500 K). V2 = V1 * (T2/T1) = 350 mL * (500/300) = 583 mL.

Question 15

Complete the following statement: In Charles's Law, the volume of a gas ________ when the ________ decreases.

Accepted Answer

According to Charles's Law, the volume of a gas decreases when the temperature decreases. This is because as the temperature of the gas decreases, the gas particles lose energy and move more slowly, causing them to take up less space and the volume of the gas to decrease.

Question 16

At 570. mm Hg and 25 °C, a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a temperature of 175 °C, if the moles are constant?

Accepted Answer

Using the combined gas law: (P1 * V1) / T1 = (P2 * V2) / T2, convert temperatures to Kelvin and solve for P2.

Question 17

The volume of a sample of gas, initially at 25 °C and 158 mL, increases to 450. mL. What is the final temperature of the sample of gas, if the pressure in the container is kept constant?

Accepted Answer

Using Charles's Law (V1/T1 = V2/T2), convert temperatures to Kelvin, solve for T2, and convert back to Celsius. The final temperature is 576 °C.

Question 18

A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15 °C. What is the volume of the bubble when it reaches the surface where the pressure is 1.0 atm and the temperature is 27 °C, if the moles are constant?

Accepted Answer

We can use the combined gas law formula to solve for the new volume:

(P1V1/T1) = (P2V2/T2)

Where:
P1 = 2.4 atm (initial pressure)
V1 = 250 mL (initial volume)
T1 = 15 °C + 273 = 288 K (initial temperature in Kelvin)
P2 = 1.0 atm (final pressure)
V2 = unknown
T2 = 27 °C + 273 = 300 K (final temperature in Kelvin)

Plugging in the values, we get:

(2.4 atm)(250 mL)/(288 K) = (1.0 atm)(V2)/(300 K)

Solving for V2:

V2 = (2.4 atm)(250 mL)(300 K)/(1.0 atm)(288 K) = 630 mL

Therefore, the volume of the bubble when it reaches the surface is 630 mL. Answer choice B is correct.

Question 19

A gas at 5.00 atm pressure was stored in a tank during the winter at 5.0 °C. During the summer, the temperature in the storage area reached 40.0 °C. What was the pressure in the gas tank then?

Accepted Answer

Using the ideal gas law, the pressure is directly proportional to the temperature in Kelvin. Convert temperatures to Kelvin (5.0 °C = 278.15 K, 40.0 °C = 313.15 K) and use the formula P1/T1 = P2/T2 to find the new pressure: (5.00 atm / 278.15 K) = (P2 / 313.15 K), solving for P2 gives approximately 5.63 atm.

Question 20

A gas contained in a steel tank has a pressure of 1.5 atm at a temperature of 320 K. What will be the gas pressure when the temperature changes to 450 K, at constant moles and volume?

Accepted Answer

Using the formula P1/T1 = P2/T2, where P is pressure and T is temperature:
P1 = 1.5 atm
T1 = 320 K
T2 = 450 K
P2 = (1.5 atm)(450 K)/(320 K) = 2.1 atm
Therefore, the gas pressure will be 2.1 atm when the temperature changes to 450 K, at constant moles and volume. The answer is D.

Quiz 8: Gases

What unit of temperature is used in gas law calculations?

An autoclave is used to sterilize surgical equipment because

The temperature of a 500. mL sample of gas increases from 150. K to 350. K. What is the final volume of the sample of gas, if the pressure and moles in the container is kept constant?

Vapor pressure can be described as

When the combined gas law is rearranged to solve for V₂, the following is the correct expression: V₂ =

A balloon is filled with helium gas. For the question(s) that follow, select the letter of the balloon diagram that corresponds to the given change in conditions. -The balloon is put into a chamber whose pressure is less than the atmospheric pressure and at atmospheric temperature.

The boiling point of water at sea level is 100 °C. At higher altitudes, the boiling point of water will be

A balloon is filled with helium gas. For the question(s) that follow, select the letter of the balloon diagram that corresponds to the given change in conditions. -The temperature is changed from 50 °C to -150 °C at constant pressure.

In Gay-Lussac's Law, the pressure of a gas increases due to an increase in temperature because

A sample of helium gas at 27.0 °C and 3.60 atm pressure is cooled in the same container to a temperature of -73.0 °C. What is the new pressure?

A gas sample in a closed, expandable container of initial volume 5.00 L was allowed to warm from 25 °C to 35 °C, at constant moles and pressure. What was its new volume?

A sample of argon gas at 300. °C and 50.0 atm pressure is cooled in the same container to a temperature of 0.00 °C. What is the new pressure?

As the temperature of a gas increases, the density of the gas will

The temperature of a 350. mL sample of gas increases from 27 °C . to 227 °C . What is the final volume of the sample of gas, if the pressure and moles in the container is kept constant?

Complete the following statement: In Charles's Law, the volume of a gas when the decreases.

At 570. mm Hg and 25 °C, a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a temperature of 175 °C, if the moles are constant?

The volume of a sample of gas, initially at 25 °C and 158 mL, increases to 450. mL. What is the final temperature of the sample of gas, if the pressure in the container is kept constant?

A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15 °C. What is the volume of the bubble when it reaches the surface where the pressure is 1.0 atm and the temperature is 27 °C, if the moles are constant?

A gas at 5.00 atm pressure was stored in a tank during the winter at 5.0 °C. During the summer, the temperature in the storage area reached 40.0 °C. What was the pressure in the gas tank then?

A gas contained in a steel tank has a pressure of 1.5 atm at a temperature of 320 K. What will be the gas pressure when the temperature changes to 450 K, at constant moles and volume?

Quiz 8: Gases

What unit of temperature is used in gas law calculations?

An autoclave is used to sterilize surgical equipment because

The temperature of a 500. mL sample of gas increases from 150. K to 350. K. What is the final volume of the sample of gas, if the pressure and moles in the container is kept constant?

Vapor pressure can be described as

When the combined gas law is rearranged to solve for V2, the following is the correct expression: V2 =

A balloon is filled with helium gas. For the question(s) that follow, select the letter of the balloon diagram that corresponds to the given change in conditions. -The balloon is put into a chamber whose pressure is less than the atmospheric pressure and at atmospheric temperature.

The boiling point of water at sea level is 100 °C. At higher altitudes, the boiling point of water will be

A balloon is filled with helium gas. For the question(s) that follow, select the letter of the balloon diagram that corresponds to the given change in conditions. -The temperature is changed from 50 °C to -150 °C at constant pressure.

In Gay-Lussac's Law, the pressure of a gas increases due to an increase in temperature because

A sample of helium gas at 27.0 °C and 3.60 atm pressure is cooled in the same container to a temperature of -73.0 °C. What is the new pressure?

A gas sample in a closed, expandable container of initial volume 5.00 L was allowed to warm from 25 °C to 35 °C, at constant moles and pressure. What was its new volume?

A sample of argon gas at 300. °C and 50.0 atm pressure is cooled in the same container to a temperature of 0.00 °C. What is the new pressure?

As the temperature of a gas increases, the density of the gas will

The temperature of a 350. mL sample of gas increases from 27 °C . to 227 °C . What is the final volume of the sample of gas, if the pressure and moles in the container is kept constant?

Complete the following statement: In Charles's Law, the volume of a gas ________ when the ________ decreases.

At 570. mm Hg and 25 °C, a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a temperature of 175 °C, if the moles are constant?

The volume of a sample of gas, initially at 25 °C and 158 mL, increases to 450. mL. What is the final temperature of the sample of gas, if the pressure in the container is kept constant?

A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15 °C. What is the volume of the bubble when it reaches the surface where the pressure is 1.0 atm and the temperature is 27 °C, if the moles are constant?

A gas at 5.00 atm pressure was stored in a tank during the winter at 5.0 °C. During the summer, the temperature in the storage area reached 40.0 °C. What was the pressure in the gas tank then?

A gas contained in a steel tank has a pressure of 1.5 atm at a temperature of 320 K. What will be the gas pressure when the temperature changes to 450 K, at constant moles and volume?

When the combined gas law is rearranged to solve for V₂, the following is the correct expression: V₂ =

Complete the following statement: In Charles's Law, the volume of a gas when the decreases.