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

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

1 mole of any gas at any pressure will always

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

exert 101.3kPa of pressure on its surroundings

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

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| By Kaemai

Kaemai

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Quizzes Created: 1 | Total Attempts: 275

Questions: 15 | Attempts: 279 | Updated: Mar 5, 2024

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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

Questions and Answers

1.

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?
- A.
  
  An increase in pressure and a decrease in volume
- B.
  
  A decrease in pressure and an increase in volume
- C.
  
  An increase in temperature and an decrease in volume
- D.
  
  An increase in temperature and an increase in volume
- E.
  
  None, every gas is ideal at STP
Correct Answer
D. 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.

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2.

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.
  
  81kPa
- B.
  
  34.427kPa
- C.
  
  34.4kPa
- D.
  
  37.87kPa
- E.
  
  37.9kPa
Correct Answer
C. 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.

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0
0
3.

Choose the false statement
- A.
  
  Gases with a large mass diffuse quickly
- B.
  
  Gases are very low density substances that interact with their surroundings through collisions
- C.
  
  Volume of a gas can be increased at constant temperature by reducing pressure
- D.
  
  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.

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4.

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

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1
0
5.

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.
- A.
  
  72.4 kPa
- B.
  
  71.2kPa
- C.
  
  144.2kPa
- D.
  
  13.6kPa
- E.
  
  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

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2
0
6.

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

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

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7.

In the formula, PV=nRT, the variable n is measured in what unit
- A.
  
  Grams
- B.
  
  K
- C.
  
  KPa
- D.
  
  Molecules
- E.
  
  Moles
Correct Answer
E. Moles

Explanation
The variable "n" in the formula PV=nRT represents the number of moles. Moles is a unit of measurement used in chemistry to quantify the amount of a substance. It is a convenient unit because it allows for the comparison of different substances based on their molecular weights. Therefore, in the given formula, "n" is measured in moles.

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8.

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

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1
0
9.

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
- A.
  
  78kPa
- B.
  
  77.5kPa
- C.
  
  79.0kPa
- D.
  
  101.3kPa
- E.
  
  Not enough information
Correct Answer
E. 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

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10.

Chemistry is (the answer is e)
- A.
  
  Awesome
- B.
  
  Challenging but awesome
- C.
  
  Really cool
- D.
  
  Fun
- E.
  
  All of the above
Correct Answer
E. 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.

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11.

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

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4
12.

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.

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4
13.

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)

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4
14.

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

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4
15.

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Quiz Created by
Kaemai

Honors Chemistry Gas Laws

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?

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

1 mole of any gas at any pressure will always

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.

Which set of variables exhibits a direct relationship?

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

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

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

Chemistry is (the answer is e)

Real gases resemble ideal gases at pressure

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

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.

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

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

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?

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?

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

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