Ch5 Lec 3 - Revision history

Bes: /* Question 2 */

2020-03-30T21:16:07Z

Question 2

2020-03-30T21:01:03Z

Question 2

2020-03-30T20:59:34Z

Question 2

2020-03-30T20:58:07Z

Question 2

2020-03-30T20:46:53Z

Question 2

2020-03-30T20:12:56Z

Question 2

2020-03-30T20:11:38Z

Question 1

2020-03-30T20:05:58Z

Ideal Gas Law Equation (Sec 5.4)

2020-03-30T20:05:03Z

Ideal Gas Law Equation (Sec 5.4)

2020-03-30T19:59:00Z

Ideal Gas Law Equation (Sec 5.4)

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 Nearly all gases behave similarly when under a set of conditions (P, V, and T). So much so that we define a set of conditions, "standard temperature and pressure" (STP) as T = 273.15 K and P = 1 atm. Under STP, the volume of 1.00 moles of gas is 22.4 L. This concept was discussed in the crash course video.
 :[[File:Screen Shot 2020-03-29 at 11.20.53 AM.png|300px|thumb|center|from Crash Course]]
 '''End of Chapter 5'''

← Older revision		Revision as of 21:01, 30 March 2020
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	: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:'''''
		+
		+
		+	Comments on Temperature: Always use Kelvin. <sup>o</sup>C + 273.15 = K

← Older revision		Revision as of 20:59, 30 March 2020
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	Nearly all gases behave similarly when under a set of conditions (P, V, and T). So much so that we define a set of conditions, "standard temperature and pressure" (STP) as T = 273.15 K and P = 1 atm. Under STP, the volume of 1.00 moles of gas is 22.4 L. This concept was discussed in the crash course video.		Nearly all gases behave similarly when under a set of conditions (P, V, and T). So much so that we define a set of conditions, "standard temperature and pressure" (STP) as T = 273.15 K and P = 1 atm. Under STP, the volume of 1.00 moles of gas is 22.4 L. This concept was discussed in the crash course video.
	:[[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]]
		+
		+	'''End of Chapter 5'''

← Older revision		Revision as of 20:58, 30 March 2020
Line 36:		Line 36:


−		+	Nearly all gases behave similarly when under a set of conditions (P, V, and T). So much so that we define a set of conditions, "standard temperature and pressure" (STP) as T = 273.15 K and P = 1 atm. Under STP, the volume of 1.00 moles of gas is 22.4 L. This concept was discussed in the crash course video.
−	~~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]]

@@ Line 29: / Line 29: @@
 Given:
-:V= 22.4 L
+:V= 22.414 L
-:n = 1.00 moles
+:n = 1.0000 moles
-:T = 298 K
+:T = 273.15 K
 :R = from above...
 '''''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]]

@@ Line 26: / Line 26: @@
 ====Question 2====
 If given the V, n, and T, which gas constant would you use if you want to calculate the pressure in "bar"?
-<div align="right">Answer: 0.08145 L*bar/(mol*K)</div>
+<div align="right">Answer: 0.08314 L*bar/(mol*K)</div>
 Given:

@@ Line 15: / Line 15: @@
 :n = 1.00 moles
 :T = 298 K
-<div align="right". Answer: 0.082057 L*atm/(mol*K)
+<div align="right">Answer: 0.082057 L*atm/(mol*K)</div>
 If the volume was not given in the question above, show how it can be calculated:
@@ Line 22: / Line 22: @@
 :T = 298 K
 :R = 0.082057 l*atm/(mol*K)
-'''''Calculate V= ? L'''''
+'''''Calculate V and make sure your work shows how the units cancel:'''''
 :[[File:Screen Shot 2020-03-29 at 11.20.53 AM.png|300px|thumb|center|from Crash Course]]

@@ Line 7: / Line 7: @@
 ''R'', the gas constant is equal to (depending on the units):
-:[[File:Screen Shot 2020-03-30 at 2.58.32 PM.png|400px]]
+:[[File:Screen Shot 2020-03-30 at 2.58.32 PM.png|300px]]
 ====Question 1====

← Older revision		Revision as of 19:59, 30 March 2020
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	:[[File:Screen Shot 2020-03-29 at 11.21.43 AM.png\|300px\|thumb\|center\|from Crash Course]]		:[[File:Screen Shot 2020-03-29 at 11.21.43 AM.png\|300px\|thumb\|center\|from Crash Course]]

−	When combining all of the gas laws, Boyles, Charles', and Avogadro's we get the ''Ideal Gas Law Equation:''	+	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:
		+	:[[File:Screen Shot 2020-03-30 at 2.58.32 PM.png\|400px]]