Gizmo Boyle & Charles Law Student Lab Sheet Question And Answers Secure HIGHSCORE
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Course
GIZMO, Rasmussen College
Institution
GIZMO, Rasmussen College
Gizmo Boyle & Charles Law Student Lab Sheet Question And Answers( Download To Score An A)
Name: ______________________________________ Date: ________________________ Student Exploration: Boyle’s Law and Charles’s Law Vocabulary: absolute zero, Boyle’s law, Charles’s law, Gay-Lussac’s law...
Prior Knowledge Question (Do this BEFORE using the Gizmo.)
A small helium tank measures about two feet (60 cm) high. Yet it can fill over 50
balloons! How can such a small tank contain enough helium to fill so many
balloons?
The small container can hold all that helium in the container because the gas in the
tank is under a lot of pressure
Gizmo Warm-up
The Boyle’s Law and Charles’s Law Gizmo shows a
container of gas. Inside, small purple spheres
represent gas molecules.
1. Observe the particles. Are they all moving at
the same speed? Yes they are all moving at
the same speed.
2. How do the particles interact with the walls and lid of the container?
The bounce off the walls and lid while providing pressure
These interactions contribute to the pressure on the walls of the container.
Pressure is defined as force per unit area. The SI units of pressure are newtons
per square meter (N/m2), or pascals (Pa).
3. Slowly drag the temperature (T) slider back and forth. (Note: In this Gizmo, the
Kelvin scale is used to measure temperature. On the Kelvin scale, 0 degrees is
absolute zero, the coldest possible temperature. Absolute zero is equal to -
273.15 °C or -459.67 °F)
A. How does the change in temperature affect the speed of the molecules? Lower the
temperature slower the molecules. Higher the temperature the faster the
molcecules.
B. How does the change in temperature affect the volume of the
container? As the temperature gets higher the pressure increases and
the lid goes higher due to the force being applied.
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, Get the Gizmo ready:
Activity A: Boyle’s Set the temperature (T) to 300 K.
law Check that the mass (m) is set to 0 kg.
Question: How does pressure affect the volume of a gas?
1. Form hypothesis: In this experiment, you will pile weights on the lid of the
container of gas. What do you think will happen as more weight is added to the
lid?
The harder it will be for the pressure to keep it up.
2. Notice: Look at the DESCRIPTION pane. What is the mass of the lid? 10 kg
How much pressure does the lid exert on the gas? 98.1 N/m2
3. Collect data: With the temperature held constant at 300 K, use the Select mass
slider to place weights on the lid. Record the pressure and volume of the gas
for each added mass.
Added mass Total mass
Pressure* Volume
on the lid (lid + added mass)
0 kg 10 kg 98.1 N/m2 2.54 m3
10 20 kg 196.2 N/m2 1.27 m3
kg
20 30 kg 294.3 N/m2 0.85 m3
kg
30 40 kg 392.4 N/m2 0.64 m3
kg
*This model does not include atmospheric pressure, which is 101,325 N/m2.
4. Analyze: As the pressure increases at constant temperature, what happens to
the volume of the gas? The volume lowers every time the pressure rises
This relationship is called Boyle’s law.
5. Calculate: Compare the pressure and volume values in your data table.
A. How did doubling the pressure change the gas volume? It lowered the
volume by half of the original
B. How did tripling the pressure change the gas volume? It lowered the
original volume by 2/4 of its value
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