# The Gas Laws

Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.

Take a look at one or more of the following sources that explain this law.  Alternatively, read chapter 1.3 in your textbook.

✍  Now apply the Law by completing these questions:

Find more questions in your textbook.

### 2. More Gas Laws

You can use the PhET simulation below to see the various changes in temperature, pressure and volume of a fixed amount of gas when you change one of these variables.

 Click to Run

A summary of the various gas laws defining the relationships between volume, temperature and pressure are found below.

V = volume in dm3
T = temperature in K
P = pressure in kPa

Note that these relationships are not given to you in the data booklet.

These laws can be represented graphically too.

✍  Write a summary in your notebook.

### 3. Kinetic Theory of Gases and the Ideal Gas Law

The kinetic theory describes a gas as a large number of submicroscopic particles (atoms or molecules), all of which are in constant rapid motion that has randomness arising from their many collisions with each other and with the walls of the container.

✍  The kinetic theory of gases is used to describe the motion and behaviour of an ideal gas.  Using your text and other relevant sources, describe the differences between an ideal gas and a real gas in your notebook.

The molar volume of any gas at STP (standard temperature and pressure) is represented below.

Warning!Warning!Warning!Warning!Warning!Warning!Warning!Warning!Warning!
Many sources quote the molar volume of a gas as 22.4 dm3.  This is using a standard pressure of 101.3 kPa NOT 100 kPa which is the new standard adopted by the IB!  Beware of past paper questions using the old value!  The new value has been used only since the 2016 exams!  If in doubt, check your data booklet – the value is quoted there as 22.7 dm3.

Combining all the equations so far, we can derive the ideal gas equation.  This is in your data booklet as is the value for R which is the ideal gas constant.  Check to make sure you know where to find these.

You will need to be able to solve problems based on these laws.  Once you feel comfortable with them and you have read and taken relevant notes from chapter 1.3 in your text, you can try the following problems.

Problems
Answers (remember that some of these might use 22.4 instead of 22.7 as the molar volume of an ideal gas at STP.)

# Stoichiometry II

#### Terminology

1. Define the following:
• solute
• solvent
• solution
• concentration
• dilute
• concentrated
1. Create a labelled diagram(s) to illustrate these six terms and upload it to the Google+ in the category 1 Stoichiometry.

#### Problems and Mixtures

1. Have a read through these worked examples on molarity (working out concentrations of solutions).
2. Go back to the Google+ and look at the diagrams other people posted.  Click the +1 button for the one you like the best and put in the comment what you like about it.
3. Now try some of the problems here yourself.
4. What is the difference between a homogenous and a heterogenous mixture? With a partner, agree on the answer to this question.  Then record a video of your agreed explanation (no longer than 30 secs) and upload it to the Google+ community under the subject 1 Stoichiometry.

#### Limiting Reagent

Refresh your memory about how reactants and products in a chemical equation are related to each other by playing this game from last lesson.

1. Define the following:
Limiting Reagent
Excess Reagent
2. Take a look at the videos posted on the Google+ and put a +1 for the one you think is the best for clarity of explanation and visual appeal!

# Stoichiometry I

Start at the beginning and work through.  If you feel confident, then move on to the next type of problem.  If you don’t get them, SEEK HELP immediately from a classmate or me!  😛

1.  Balancing equations – Here you will find 4 different worksheets with practise questions on them.  The answers are also there.  Practise until you feel more confident.  Still stuck?  Want more practice?  Try this simulation below.

Here you will get a section explaining how to convert between moles and number of particles.  Then there are some problems to try.  You can find the page here.

3.  Moles to mass problems – Here you will find a few calculations to practise with the answers.  You can find it here.

4.  Stoichiometric relationships in equations!   Play with the simulation below!  You must make it through all 3 levels of the game with 100% correct before moving on to the next section.

5.  For more problems, tutorials and general help with the mole, you can use this useful site here.  This Crash Course video below is a 12 minute summary of Stoichiometry!

# Revision Package for Topic 1

Click HERE to go to a folder containing revision materials for Topic 1 Quantitative Chemistry.

Open the first document for syllabus details and links to practise questions and the marks schemes that go with them!

# Stoichiometery – Gas Relationships Simulation!

A great simulation for looking at the relationship between temperature, pressure and volume.

If you have trouble getting it to work, try using safari or firefox instead of chrome and make sure you have java 7 installed.

 Click to Run