1 mole of any gas at any pressure will always

contain 6.$$02x10^23$$ molecules

exert 101.3kPa of pressure on its surroundings

Choose the false statement

Gases with a large mass diffuse quickly

Gases are very low density substances that interact with their surroundings through collisions

Volume of a gas can be increased at constant temperature by reducing pressure

Gases behave as ideal gases at all temperatures

A system of gases is made up of 1.00mol CO2 and 2.00mol O2 at STP, which of the following changes would result in the system behaving more like an ideal gas?

An increase in temperature and an increase in volume

An increase in pressure and a decrease in volume

A decrease in pressure and an increase in volume

An increase in temperature and an decrease in volume

none, every gas is ideal at STP

Compared to the number of moles of O2 there are in a sample the number of atoms in the sample

is 1.$$204x10^24$$ times larger

Honors Chemistry Gas Laws

Reviewed by Editorial Team

The ProProfs editorial team is comprised of experienced subject matter experts. They've collectively created over 10,000 quizzes and lessons, serving over 100 million users. Our team includes in-house content moderators and subject matter experts, as well as a global network of rigorously trained contributors. All adhere to our comprehensive editorial guidelines, ensuring the delivery of high-quality content.

Learn about Our Editorial Process

| By Kaemai

Kaemai

Community Contributor

Quizzes Created: 1 | Total Attempts: 370

| Attempts: 370

Questions

Feedback

During the Quiz End of Quiz

Difficulty

Easy First Hard First Sequential

Share on Facebook Share on Twitter Share on Whatsapp Share on Pinterest Share on Email Copy to Clipboard Embed on your website

1/15 Questions

In the formula, PV=nRT, the variable n is measured in what unit
- Grams
- K
- KPa
- Molecules
- Moles

About This Quiz

This quiz should give a pretty good representation of your understanding, and from what I saw yesterday it seemed as though you get this stuff pretty well. If you get any questions wrong or would like more information check the explanations to see where you went wrong or what you were missing. I tried to tailor it specifically to the subjects you were having trouble with so it might be a little annoying but that makes it all the more helpful. Hope this helps, if you have any questions email me. Kareem

2.

Chemistry is (the answer is e)
- Awesome
- Challenging but awesome
- Really cool
- Fun
- All of the above
Correct Answer

A. All of the above

Explanation

This question is asking for a description of chemistry. The answer "all of the above" suggests that chemistry is all of the options listed - awesome, challenging but awesome, really cool, and fun. In other words, chemistry is considered to be an amazing subject that can be both challenging and enjoyable.

Rate this question:
3.

The relationship between two variables would be if an increase in one, resulted in an increase in the other

Correct Answer
direct
directly proportional
proportional

Explanation
The answer "direct, directly proportional, proportional" is correct because all three terms describe a relationship between two variables where an increase in one variable leads to an increase in the other variable. These terms can be used interchangeably to indicate that the variables change in the same direction and at a consistent rate.

Rate this question:
4.

Avogadro's number (6.02x10^23), is the number of that make up one mole of a substance.

Correct Answer
molecules
particles

Explanation
this is just a simple recap of what the number means

Rate this question:
5.

Which set of variables exhibits a direct relationship?
- P , V
- V , T
Correct Answer

A. V , T

Explanation

When V increases T increases , but when P increases V decreases

Rate this question:
6.

The is the quotient of the number of moles of a substance in a sample, divided by the total number of moles in the sample.

Correct Answer
mole fraction
mole ratio

Explanation
good to know what its called but more important to know that its used in determining partial pressure.(when you multiply the mole fraction by the total pressure)

Rate this question:
7.

Real gases resemble ideal gases at pressure

Correct Answer
low
small

Explanation
low pressure means a greater distance between particles, making the gas act more like an ideal gas

Rate this question:
8.

1 mole of any gas at any pressure will always
- Occupy 22.4L of space
- Contain 6.02x10^23 molecules
- Behave like an ideal gas
- Exert 101.3kPa of pressure on its surroundings
Correct Answer

A. Contain 6.02x10^23 molecules

Explanation

B must always be true for the sample to be 1 mole of gas, all the other choices can vary with pressure

Rate this question:

1
9.

A 11.0mol mixture of gases at 108.2 kPa is composed of 3.00mol He, 2.00mol H₂, 3.50mol O₂, and 1.50mol CO₂. What is the partial pressure of O₂?
- 81kPa
- 34.427kPa
- 34.4kPa
- 37.87kPa
- 37.9kPa
Correct Answer

A. 34.4kPa

Explanation

For calculating partial pressure you first find the mole ratio, in this case(3.50mol O2/10.0mol total), and then multiply by the total pressure to determine the pressure resulting from oxygen. Mind your significant figures.

Rate this question:

0
10.

Choose the false statement
- Gases with a large mass diffuse quickly
- Gases are very low density substances that interact with their surroundings through collisions
- Volume of a gas can be increased at constant temperature by reducing pressure
- Gases behave as ideal gases at all temperatures
Correct Answer

A. Gases with a large mass diffuse quickly

Explanation

This is a reference to the formula for relative rates of diffusion that shows larger mass means lower rates of diffusion, just remmber to write the formula down on the test and understand what the variables are.

Rate this question:
11.

A system of gases is made up of 1.00mol CO₂ and 2.00mol O₂ at STP, which of the following changes would result in the system behaving more like an ideal gas?
- An increase in pressure and a decrease in volume
- A decrease in pressure and an increase in volume
- An increase in temperature and an decrease in volume
- An increase in temperature and an increase in volume
- None, every gas is ideal at STP
Correct Answer

A. An increase in temperature and an increase in volume

Explanation

Fairly simple ideal gas properties, increasing the volume decreases the pressure, decreased pressure and increased temperature reduce density bringing particles farther apart making them interact less.

Rate this question:
12.

When a 1.00L sample of N2 at 43.0kPa and 1.00L sample of O2 at 29.4kPa are mixed in a 1.00L container what is the resulting total pressure.
- 72.4 kPa
- 71.2kPa
- 144.2kPa
- 13.6kPa
- 86kPa
Correct Answer

A. 72.4 kPa

Explanation

To find the resulting total pressure when the two gases are mixed, we can use Dalton's Law of Partial Pressures, which states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of each individual gas.
Mathematically, it can be represented as:
Total Pressure = Partial Pressure of N2 + Partial Pressure of O2
Given: Partial Pressure of N2 (P(N2)) = 43.0 kPa Partial Pressure of O2 (P(O2)) = 29.4 kPa
Total Pressure = 43.0 kPa + 29.4 kPa Total Pressure = 72.4 kPa

Rate this question:

2
13.

Air is a mixture of gases which is composed primarily of N₂, more specifically it is 76.5% N₂ by mass, if atmospheric pressure is 101.3kPa what is the partial pressure due to N₂
- 78kPa
- 77.5kPa
- 79.0kPa
- 101.3kPa
- Not enough information
Correct Answer

A. Not enough information

Explanation

Even though you know the percentage N2 by mass, without knowing what else is in the system and how much of it there is, it is impossible to get the mole fraction of N2

Rate this question:
14.

Compared to the number of moles of O₂ there are in a sample the number of atoms in the sample
- Is twice as much
- Is 6.02x10^23 times larger
- Is half as much
- Is 1.204x10^24 times larger
- Just as large
Correct Answer

A. Is 1.204x10^24 times larger

Explanation

Okay so this one is a little tricky, but its actualy quite simple, for every mole there are 6.02x10^23 molecules and for every molecule there are two atoms. I just wanted to demonstrate how the question could be worded to make it harder than it really is.

Rate this question:

1
15.

This is just for feedback, so feel free to write what you thought about the quiz. (length, difficulty, wording)

Quiz Review Timeline (Updated): Mar 5, 2024 +

Our quizzes are rigorously reviewed, monitored and continuously updated by our expert board to maintain accuracy, relevance, and timeliness.

Current Version
Mar 05, 2024

Quiz Edited by
ProProfs Editorial Team
Feb 21, 2010

Quiz Created by
Kaemai

Honors Chemistry Gas Laws

In the formula, PV=nRT, the variable n is measured in what unit

Quiz Preview

Chemistry is (the answer is e)

The relationship between two variables would be if an increase in one, resulted in an increase in the other

Avogadro's number (6.02x10^23), is the number of that make up one mole of a substance.

Which set of variables exhibits a direct relationship?

The is the quotient of the number of moles of a substance in a sample, divided by the total number of moles in the sample.

Real gases resemble ideal gases at pressure

1 mole of any gas at any pressure will always

A 11.0mol mixture of gases at 108.2 kPa is composed of 3.00mol He, 2.00mol H2, 3.50mol O2, and 1.50mol CO2. What is the partial pressure of O2?

Choose the false statement

A system of gases is made up of 1.00mol CO2 and 2.00mol O2 at STP, which of the following changes would result in the system behaving more like an ideal gas?

When a 1.00L sample of N2 at 43.0kPa and 1.00L sample of O2 at 29.4kPa are mixed in a 1.00L container what is the resulting total pressure.

Air is a mixture of gases which is composed primarily of N2, more specifically it is 76.5% N2 by mass, if atmospheric pressure is 101.3kPa what is the partial pressure due to N2

Compared to the number of moles of O2 there are in a sample the number of atoms in the sample

This is just for feedback, so feel free to write what you thought about the quiz. (length, difficulty, wording)

A 11.0mol mixture of gases at 108.2 kPa is composed of 3.00mol He, 2.00mol H₂, 3.50mol O₂, and 1.50mol CO₂. What is the partial pressure of O₂?

A system of gases is made up of 1.00mol CO₂ and 2.00mol O₂ at STP, which of the following changes would result in the system behaving more like an ideal gas?

Air is a mixture of gases which is composed primarily of N₂, more specifically it is 76.5% N₂ by mass, if atmospheric pressure is 101.3kPa what is the partial pressure due to N₂

Compared to the number of moles of O₂ there are in a sample the number of atoms in the sample