Gas+Laws

__**Directions:**__ a) list and define all vocabulary from this chapter. b) type at least 4 sample problems with step-by-step directions of how to solve the problem; list the correct answers (if your chapter doesn't have math, there are still problems and concepts we learned.) c) link at least 3 websites for additional resources to help with studying d) develop your own LEQ questions for the section - what did you think were the key points we learned? e) Once your page is done, visit 4 other chapters and answer their LEQ's. (This can be done on a separate piece of paper.)

gas: assume the volume and the shape of it's container. Pressure: force/area atm=atmosphere torr= torrance Pa= pascal Boyles law- at constant temp the volume changes as pressure changes. As pressure increases volume decreases. Charles law- At constant pressure, volume changes as temperature does. As temperature increases volume increases. STP- (standard temp and pressure) 0 degrees celcius, 273.13 K, 1 atm Partial pressure- a portion of the total pressure Diffusion- movement of one gas through another Effusion- gas escapes its container through a tiny hole into an evacuated space.
 * __Vocabulary-__**

__**Bolyles Law-**__ constant temperature and constant amount of gas. P1xV1=P2xV2

P1= (273 atm x .5862 L)/ 1 L = 160 atm

1) divide the volume of the the first solution into the second solution but do not solve 2) multiply the second volume and pressure of the second solution 3) now divide the fraction that you have of (atm x L)/L and cross out the L just to get the pressure. 4) remember sig figs The same thing goes for volume in this.

Temperature must be in Kalvin t(C)+273.15=Kalvin V1/T1=V2/T2
 * __Charles and Gay-Lussac Law-__**

819 mL/ 294.15 K= x/273 K x= 760

1) divide the fraction that you have of so you have mL x K 2) Multiply th denominator of the fraction you have to cross out Kalvin and just get mL 3) use sig figs to get the value

__**Ideal Gas Laws-**__ PV=nRT R is the gas' contant used when discussing a single gas i non-changing environment.

The condition O C and 1 atm are called the standard temperature and pressure. (STP)

Experiments show that at STP, 1 mole of an ideal gas occupies 22.414 L

R=PV/nT=(1 atm)(22.414 L)/(1 atm)(273.15 K) R= 0.082057 atm/(molxK) or 8.314 L x kPa/(molxK)

(2 mol x 0.0821 (L x atm)/(mol x K) x 273.15 K)/ 1 atm = 44.45 ml

1) multiply the top to get the top value. After you do that and cross things out you should get (L x atm)/atm 2) Divide by the bottom number to get just the volume of the solution ( you can also do this for pressure) 3) If in L pt in mL 4) don't forget sig figs

__**Combi****ned Gas Laws-**__ Happens when n and R are constant (P1xV1)/T1=(P2xV2)/T2

(7.00 L x 625 kPa)/ 420 K= (1.25 L x X kPa)/ 350 K X= 2920 kPa

1) Multiply the volume 1 and pressure 1 2) Divide the temperature 1 3) Multiply the temperature 2 into the number that you multiplied and divided. 4) Then divided the volume of the second solution into the first solution 5) don't forget to use sig figs

__**Dalton's Law-**__ P1+P2=Ptotal consider a case in which two gases are in a container of volume V. PA=(n+RT)/V PB=(n+RT)/V PT=PA+PB

7.8 g x (mol CO2/ 43.99 g) = .1773 moles P= (.1773 moles x .0821 (atm x L)/(mol x K) x 300.15 K)/ 4.0 L P= 1.1 atm

particle: 1.09 x 760= 828.4 torr total: 838.4 + 740 = 1596 torr

1) do the same thing you did for ideal gas laws to get the pressure of the substance 2) if the second pressure is in some other pressure, convert to that pressure 3) add or subtract the amount to get the total pressure of the substance 4) don't forget sig figs


 * __Graham's Law-__**

rate 1/rate 2 = square root( gas 1/gas 2) gas 1 are alway the lighter gas gas 2 are the slower and heavier gases.

Kinetic Energy=1/2mv^2 has the same temperature
 * comparing the motion of __gases__

http://hyperphysics.phy-astr.gsu.edu/hbase/kinetic/idegas.html http://misterguch.brinkster.net/gaslaws.html http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch4/gaslaws3.html
 * __Websites-__**