Difference between revisions of "Ch5 Lec 3"
| Line 29: | Line 29: | ||
Given: | Given: | ||
| − | :V= 22. | + | :V= 22.414 L |
| − | :n = 1. | + | :n = 1.0000 moles |
| − | :T = | + | :T = 273.15 K |
:R = from above... | :R = from above... | ||
'''''Calculate the pressure in bar and make sure your work shows how the units cancel:''''' | '''''Calculate the pressure in bar and make sure your work shows how the units cancel:''''' | ||
| Line 37: | Line 37: | ||
| − | + | As highlighted in | |
:[[File:Screen Shot 2020-03-29 at 11.20.53 AM.png|300px|thumb|center|from Crash Course]] | :[[File:Screen Shot 2020-03-29 at 11.20.53 AM.png|300px|thumb|center|from Crash Course]] | ||
Revision as of 20:46, 30 March 2020
in progress...
Ideal Gas Law Equation (Sec 5.4)
When combining all of the gas laws, Boyles, Charles', and Avogadro's we get the Ideal Gas Law Equation: As with any mathematical relationship/equation, if there are 5 variables (P, V, n, R, T) all you need to know is 4 of them and the 5th can be calculated.
R, the gas constant is equal to (depending on the units):
Question 1
If given the following data, which gas constant would you use?
- P = 1.12 atm
- V= 2.45 L
- n = 1.00 moles
- T = 298 K
If the volume was not given in the question above, show how it can be calculated:
- P = 1.12 atm
- n = 1.00 moles
- T = 298 K
- R = 0.082057 l*atm/(mol*K)
Calculate V and make sure your work shows how the units cancel:
Question 2
If given the V, n, and T, which gas constant would you use if you want to calculate the pressure in "bar"?
Given:
- V= 22.414 L
- n = 1.0000 moles
- T = 273.15 K
- R = from above...
Calculate the pressure in bar and make sure your work shows how the units cancel:
As highlighted in
