Embedded Files
Lesson Instructions
Lesson Instructions
Review the learning goals and success criteria for Topic 2: Gases and Pressure Changes [Boyles Law].
Review the minds on, action, and consolidation sections of the lesson, completing any tasks as outlined.
Complete the fill-in-the-blanks handouts that have been provided to you. They have been linked below.
Practice and apply what you've learned by completing the practice tasks outlined at the end of the lesson.
Learning Goals
Learning Goals
I am learning to ...
convert units of pressure and temperature.
use Boyle’s Law, P1V1 = P2V2 , to determine the effect of changing pressure or volume at constant temperature.
Minds On
Minds On
Have you ever wondered – Why does soda fizz?
Have you ever wondered – Why does soda fizz?
Find out why soda fizzes out of the can and what this has to do with Boyle's law!
Action
Action
Gases and Pressure Changes
Gases and Pressure Changes
Gas Pressure (P)
Gas Pressure (P)
Is the result of constantly moving gas molecules striking the inside surface of their container.
Converting Units of Gas Pressure
Converting Units of Gas Pressure
The following table is used to convert between different units of gas pressure:
Example
Example
Convert 98.3 kPa into atmospheres.
Practice
Practice
Now that you've learned how to convert between different units of gas pressure, convert the following units of pressure:
(a) Convert 1.23 atm to mm Hg
(b) Convert 15.3 psi to kPa
Kelvin Temperature Scale
Kelvin Temperature Scale
This scale was designed so that 0 Kelvin is the temperature at which a substance possesses no kinetic energy.
0 Kelvin = ABSOLUTE ZERO
Absolute Zero = 0 K = -273.15 °C
Absolute Zero = 0 K = -273.15 °C
Example
Example
Convert the following temperatures:
(a) 35.2°C to Kelvin
(b) 402 K to °C
Boyle's Law
Boyle's Law
Boyle's Law states that decreasing the volume of the container will increase the number of collisions and thus causes an increase in pressure.
Boyle’s Law states that the volume of a gas is inversely proportional to the pressure at constant temperature:
P1V1 = P2V2
P1V1 = P2V2
Example
Example
If a balloon containing 500. mL of helium gas under 1.50 atm pressure is released to 1.00 atm, what is the new volume?
Example
Example
A gas occupies 15.3 L at 0.560 atm. What is the pressure, in kPa, if the volume is expanded to 19.2 L?
This lesson is now complete. Consolidate your learning by evaluating the self-check below and the assigned practice questions.
Self-Check
(This is a self-assessment of your learning – you do not need to submit this).Self-Check
How prepared am I to start my homework? Can I ...
convert units of pressure and temperature?
use Boyle’s Law, P1V1 = P2V2 , to determine the effect of changing pressure or volume at constant temperature?
Practice
Practice
Using your textbook, complete the following questions:
p510 #9 a-c
p518 #16
p514 #5-8
p515 #5bd, 6, 13
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