Question 1

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

The answer of The volume of a sample of gas,...

Question 2

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 caused by the individual molecules of the liquid leaving the surface and entering the gas phase, creating a dynamic equilibrium between the liquid and the gas.

Question 3

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 4

A sample of argon 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 at 300. °C...

Question 5

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

Accepted Answer

As the temperature of a gas increases, the average kinetic energy of the gas molecules also increases, causing them to move faster and spread out more. This increase in volume (assuming constant pressure) results in a decrease in density.

Question 6

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

Accepted Answer

Rearranging the combined gas law, we get: P1V1/T1 = P2V2/T2 Multiplying both sides by P2V1: P2V1P1V1/T1 = P2V2P1V1/T2 Simplifying: V1/T1 = V2/T2 Rearranging: V1T2 = V2T1 Now, to solve for V₂: V₂ = V1T2/T1 Substituting from earlier: V₂ = (P2V1/T1)T2/T1 Simplifying: V₂ = (P2V1/T1)(T2/T1) V₂ = (P2V1T2)/(T1^2) Since P1V1/T1 = P2V2/T2: P2V1 = P1V1(T2/T1) Substituting: V₂ = (P1V1T2)/(T1^2) = (P₁V1T2)/(T1^2) = P₁V1T2/(P₂T1) = P₁V1(T2/P₂T1)

Question 7

A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure was 760 torr?

Accepted Answer

Use the combined gas law equation:

(P1V1/T1) = (P2V2/T2)

P1 = 740 torr, V1 = 500 mL, T1 = 25 + 273 = 298 K (temperature must be in Kelvin)

P2 = 760 torr, T2 = 50 + 273 = 323 K

Substitute the values:

(740 torr x 500 mL) / 298 K = (760 torr x V2) / 323 K

Solve for V2:

V2 = (740 torr x 500 mL x 323 K) / (760 torr x 298 K) = 530 mL

Therefore, the new volume of the nitrogen gas is 530 mL.

Question 8

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 is directly proportional to its temperature at a constant pressure and quantity of gas. This means that as the temperature of the gas decreases (holding pressure and quantity constant), the volume will also decrease. Therefore, the correct answer is D) decreases; temperature.

Question 9

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?

Accepted Answer

We can use the combined gas law to solve this problem:

(P1V1/T1) = (P2V2/T2)

where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2, V2, and T2 are the final pressure, volume, and temperature.

Plugging in the given values:

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

Solving for V2:

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

Therefore, the volume of the bubble when it reaches the surface is 630 mL, which corresponds to choice (B).

Question 10

A gas sample in a closed, expandable container of initial volume 5.00 L was allowed to warm from 25 °C to 35 °C. 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.
We can use the formula V2 = V1(T2/T1), where V1 = initial volume = 5.00 L, T1 = initial temperature = 25°C + 273 = 298 K, T2 = final temperature = 35°C + 273 = 308 K.
Plugging in the values, we get V2 = 5.00 L x (308 K/298 K) = 5.17 L. Therefore, the new volume of the gas is 5.17 L.

Question 11

At STP, what is the volume of 4.50 moles of nitrogen gas?

Accepted Answer

Using the ideal gas law, PV = nRT, we can solve for V (volume) at STP (standard temperature and pressure: 0°C and 1 atm).
At STP, R = 0.08206 L*atm/(mol*K).
So V = (nRT)/P = (4.50 mol)(0.08206 L*atm/(mol*K))(273 K)/1 atm = 100.19 L ≈ 101 L. Therefore, the answer is choice C.

Question 12

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?

Accepted Answer

Using the ideal gas equation, PV = nRT, we can solve for the new pressure at the new temperature:
P1/T1 = P2/T2
1.5/320 = P2/450
P2 = (1.5/320) * 450
P2 = 2.1 atm

Question 13

What unit of temperature is used in gas law calculations?

Accepted Answer

Gas law calculations typically use the Kelvin (K) temperature scale because it is an absolute scale where 0K represents the lowest possible temperature (absolute zero) and all temperatures are positive values. This is important for gas law calculations because temperatures must be in absolute units to accurately calculate the behavior of gases.

Question 14

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 affected by atmospheric pressure. At higher altitudes, atmospheric pressure is lower, which means it takes less energy to convert water into gas. Therefore, the boiling point is lower at higher altitudes.

Question 15

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

The answer of A gas at 5.00 atm pressure was...

Question 16

An autoclave is used to sterilize surgical equipment because

Accepted Answer

The answer of An autoclave is used to sterilize surgical...

Question 17

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, the pressure of a gas is directly proportional to its temperature when the volume is constant. As temperature increases, the kinetic energy of the gas molecules also increases, causing them to move faster and collide more frequently with the walls of the container. This increased collision frequency leads to a higher pressure. Therefore, Option B, "the molecules strike the walls of the container more often," is the correct answer.

Question 18

At STP, how many moles of helium would occupy 1.00 L?

Accepted Answer

At STP (Standard Temperature and Pressure), 1 mole of any ideal gas occupies 22.4 liters. Therefore, to find out how many moles of helium would occupy 1.00 L, you divide 1.00 L by 22.4 L/mole, which gives approximately 0.0446 moles.

Question 19

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 in the container is kept constant?

Accepted Answer

According to Charles's Law, V1/T1 = V2/T2. Solving for V2 gives V2 = V1 * (T2/T1) = 500 mL * (350 K / 150 K) = 1166.67 mL, which rounds to 1170 mL.

Question 20

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?

Accepted Answer

Using the combined gas law, we can solve for the final pressure:P1V1/T1 = P2V2/T2(570 mmHg)(2270 mL)/(25 °C + 273) = P2(1250 mL)/(175 °C + 273)P2 = 1560 mmHg

Quiz 7: Gases

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?

Vapor pressure can be described as

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.

A sample of argon 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 __________.

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

A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure was 760 torr?

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

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?

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

At STP, what is the volume of 4.50 moles of nitrogen gas?

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?

What unit of temperature is used in gas law calculations?

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

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?

An autoclave is used to sterilize surgical equipment because

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

At STP, how many moles of helium would occupy 1.00 L?

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 in the container is kept constant?

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?

Quiz 7: Gases

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?

Vapor pressure can be described as

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.

A sample of argon 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 __________.

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

A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure was 760 torr?

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

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?

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

At STP, what is the volume of 4.50 moles of nitrogen gas?

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?

What unit of temperature is used in gas law calculations?

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

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?

An autoclave is used to sterilize surgical equipment because

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

At STP, how many moles of helium would occupy 1.00 L?

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 in the container is kept constant?

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?

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.