Thursday, May 7, 2020

SCH 3U - Combined Gas Law & Dalton's Law of Partial Pressure


STP & SATP
Chemists do experiments under distinct conditions.  Often, a certain set of conditions gets used quite often, so chemists have created a shortcut method of indicating those conditions.  Be familiar with STP and SATP, as they will pop up in gas law questions.

Standard Temperature & Pressure (STP):
standard temperature = 0°C or 273.15 K
standard pressure = 101.325 kPa

Standard Ambient Temperature & Pressure (SATP):
standard ambient temperature = 25.00°C or 298.15 K
standard ambient pressure = 100.0 kPa



Combined Gas Law
Recall that V 1/P, V T
So V T/P or PV T

For the gas at initial conditions, P1V1/T1 = k
For the gas at final conditions, P2V2/T2 = k

P1V1/T1 = P2V2/T2

ex. What pressure is required to put 212 L of chlorine gas, originally at STP, into a 52 L tank at 12.4°C?

P1 = 101.325 kPa                                                           P1V1/T1 = P2V2/T2
V1 = 212 L                                   101.325 kPa(212 L)/273.15 K = P2(52 L)/285.5 K
T1 = 0 + 273.15 K = 273.15 K                                                 P2 = 431.1 kPa
P2 = ?                                                         the pressure is 430 kPa.
V2 = 52 L
T2 = 12.4 + 273.15 = 285.5 K



Dalton’s Law of Partial Pressures
The total pressure of a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases.

Ptotal = p1 + p2 + p3 + ---

ex. A flask contains an air mixture that has oxygen at a partial pressure of 28 kPa and nitrogen at a partial pressure of 110 kPa.  What is the total pressure in the tank?

p1 = 28 kPa                              P = p1 + p2
p2 = 110 kPa                                = 28 kPa + 110 kPa
P = ?                                            = 138 kPa
                                      the total pressure 138 kPa.


Homework:
Practice p. 542 # 1-3, 8
Learning Check p. 557 # 9-12



 
 

 
 
 
Student Questions:

 1.  Can you do p. 557 # 9, 10 & 12?

Sure can:



2.  Do some more...

3.  Seriously, miss, just do them all...