Question

Post-Lab Reflection Questions

Answer the reflection questions using what you have learned from the lesson and your experimental data. It will be helpful to refer to your chemistry journal notes. Answer questions in complete sentences.
1. Why was the line of best fit method used to determine the experimental value of absolute zero?

2. Which gas law is this experiment investigating? How does your graph represent the gas law under investigation?

3. Using your knowledge of the kinetic molecular theory of gases, describe the relationship between volume and temperature of an ideal gas. Explain how this is reflected in your lab data.

4. Pressure and number of moles remained constant during this experiment. If you wanted to test one of these variables in a future experiment, how would you use your knowledge of gas laws to set up the investigation?

Answer 1

Here is an alternative answer for question 4!

Step-by-step explanation:

To test these variables you would want to use the other variables such as temperature to be changed, meaning that temperature would decrease and increase, thus changing the amounts/number of moles and pressure. This is the best thing to do since at a constant temperature, according to gas laws, volume, pressure, and amount of moles all stay constant as well, so temperature should be the variable to change, decreasing and increasing, thus increasing and decreasing the pressure, volume, and amount of moles.

I really hope this helps you!

*please do not copy and paste tho, think abt academic integrity...YOUR BETTER THAN THIS*

Also I'm in honors chem so don't worry this is correct, i got you bestie :)

Answer 2

1. Why was the line of best fit method used to determine the experimental value of absolute zero?

The line of best fit method is used to determine the experimental value, because it most accurately shows where the line crosses the x-axis.

2. Which gas law is this experiment investigating? How does your graph represent the gas law under investigation?

This investigation is experimenting the “Ideal Gas Law”. This law by Gay-Lussac shows that when the volume in a container of a gas is held constant, while the temperature is increased, the pressure will also increase.

3. Using your knowledge of the kinetic molecular theory of gases, describe the relationship between volume and temperature of an ideal gas. Explain how this is reflected in your lab data.

As temperature increases, volume increases when pressure is held constant. As seen in the chart, as the temperature increases the volume in each gas also increases slightly.

4. Pressure and number of moles remained constant during this experiment. If you wanted to test one of these variables in a future experiment, how would you use your knowledge of gas laws to set up the investigation?

Supposedly at a constant temperature, the gas volume and pressure stay constant. Therefore, the amount of moles also remains constant. So perhaps, the temperature could fluctuate, meaning it will not only increase or decrease, but do both. This will avoid consistency and prove the Ideal Gas Law to be true.

Step-by-step explanation: