Difference between revisions of "Ch5 Lec 2"
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:If you look on the webpage, you will see that there is an active link to the Exam 2 on Friday April 3. I suggest you have a look at that link to give you more information about the format of the exam. | :If you look on the webpage, you will see that there is an active link to the Exam 2 on Friday April 3. I suggest you have a look at that link to give you more information about the format of the exam. | ||
| − | Note that the chapter 5 outline was given in Lecture 1. I have chosen to focus our attention on only the first 4 sections. | + | Note that the chapter 5 outline was given in Lecture 1. I have chosen to focus our attention on only the first 4 sections of chapter 5. |
The following two sections are both discussed in the following Crash Course...please note that these crash course videos provide a huge amount of information in a short time period. This one in particular goes into a lot of the background histroy, which is an important thing to know, but will not be on the exam...have a look at: | The following two sections are both discussed in the following Crash Course...please note that these crash course videos provide a huge amount of information in a short time period. This one in particular goes into a lot of the background histroy, which is an important thing to know, but will not be on the exam...have a look at: | ||
| Line 8: | Line 8: | ||
===Gas laws (Sec 5.3)=== | ===Gas laws (Sec 5.3)=== | ||
| − | + | READ this section... | |
| − | === | + | Summary: |
| + | :[[File:Screen Shot 2020-03-29 at 11.08.15 AM.png|400px|thumb|center|from Crash Course video]] | ||
| + | |||
| + | ====Boyle's Law Question==== | ||
| + | :So if you have a container of gas at 1.0 atm pressure (P<sub>1</sub>) and 1.0 L volume (V<sub>1</sub>)...if the volume is changed to 0.5 L (P<sub>2</sub>), then what happens to the pressure? | ||
| + | ::Use: P<sub>1</sub>V<sub>1</sub>=P<sub>2</sub>V<sub>2</sub>; | ||
| + | |||
| + | <div align="right"> Answer: 2.0 atm </div> | ||
| + | |||
| + | ====Charles' Law Question 1==== | ||
| + | :So if you have a balloon of gas at a temperature of 298 K (T<sub>1</sub>) and 1.0 L volume (V<sub>1</sub>)...if the temperature is changed to 330 K (T<sub>2</sub>) what is the new volume? | ||
| + | ::Use: V<sub>1</sub>/T<sub>1</sub>=V<sub>2</sub>/T<sub>2</sub>; | ||
| + | |||
| + | <div align="right"> Answer: 1.11 L </div> | ||
| + | |||
| + | ====Charles' Law Question 2==== | ||
| + | :In Charles Law Question 1, we were dealing with a balloon; a balloon has movable walls and hence the volume can change. If you do the same experiment in a jar (non movable walls) then the pressure will change. | ||
| + | :So if you have a 1.0 L jar of gas at a temperature of 298 K (T<sub>1</sub>) and a pressure of 1.0 atm (P<sub>1</sub>)...if the temperature is changed to 330 K (T<sub>2</sub>) what is the new pressure? | ||
| + | ::Use: P<sub>1</sub>/T<sub>1</sub>=P<sub>2</sub>/T<sub>2</sub>; | ||
| + | |||
| + | <div align="right"> Answer: 1.11 atm </div> | ||
| + | |||
| + | ====Avogadro's Law Question 1==== | ||
| + | :If you have 1.0 moles (n<sub>1</sub>) of gas and in a balloon with a volume of 22.4 L (V<sub>1</sub>), what is the volume of the balloon once 0.25 moles (n<sub>2</sub>) of gas is released? | ||
| + | ::Use: V<sub>1</sub>/n<sub>1</sub>=V<sub>2</sub>/n<sub>2</sub>; | ||
| + | |||
| + | <div align="right"> Answer: 16.8 L </div> | ||
| + | |||
| + | '''''There is a WebAssign available now (Monday, 8 am) for you to practice gas law questions...''''' | ||
Latest revision as of 03:02, 30 March 2020
Greetings,
- If you look on the webpage, you will see that there is an active link to the Exam 2 on Friday April 3. I suggest you have a look at that link to give you more information about the format of the exam.
Note that the chapter 5 outline was given in Lecture 1. I have chosen to focus our attention on only the first 4 sections of chapter 5.
The following two sections are both discussed in the following Crash Course...please note that these crash course videos provide a huge amount of information in a short time period. This one in particular goes into a lot of the background histroy, which is an important thing to know, but will not be on the exam...have a look at:
Gas laws (Sec 5.3)
READ this section...
Summary:
Boyle's Law Question
- So if you have a container of gas at 1.0 atm pressure (P1) and 1.0 L volume (V1)...if the volume is changed to 0.5 L (P2), then what happens to the pressure?
- Use: P1V1=P2V2;
Answer: 2.0 atm
Charles' Law Question 1
- So if you have a balloon of gas at a temperature of 298 K (T1) and 1.0 L volume (V1)...if the temperature is changed to 330 K (T2) what is the new volume?
- Use: V1/T1=V2/T2;
Answer: 1.11 L
Charles' Law Question 2
- In Charles Law Question 1, we were dealing with a balloon; a balloon has movable walls and hence the volume can change. If you do the same experiment in a jar (non movable walls) then the pressure will change.
- So if you have a 1.0 L jar of gas at a temperature of 298 K (T1) and a pressure of 1.0 atm (P1)...if the temperature is changed to 330 K (T2) what is the new pressure?
- Use: P1/T1=P2/T2;
Answer: 1.11 atm
Avogadro's Law Question 1
- If you have 1.0 moles (n1) of gas and in a balloon with a volume of 22.4 L (V1), what is the volume of the balloon once 0.25 moles (n2) of gas is released?
- Use: V1/n1=V2/n2;
Answer: 16.8 L
There is a WebAssign available now (Monday, 8 am) for you to practice gas law questions...