warm up2-7-14 1.what is stp? 2. how much space does 1 mole of hydrogen gas occupy at stp? 3. how...
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Warm UpWarm Up 2-2-7-147-14
1.What is STP?
2. How much space does 1 mole of hydrogen gas occupy at STP?
3. How many torr is in 5 atm?4. Convert 30 Celsius to Kelvin.
Agenda-Pick up binders (40pts)-Notes Chp 12-3 (gas laws)-WS The gas law
HomeworkQuiz next class
12-312-3The Gas LawsThe Gas Laws
Mathematical relationships between volume, temperature,
pressure and amount of gas
Combined Gas LawCombined Gas Law:: Pressure, Volume Pressure, Volume
&Temperature&Temperature• Combines all three gas laws into one
equation!!• Memorize this equation!!!
P1V1=
P2V2
T1 T2Remember: all
temperatures must be in Kelvin!!!
Combined LawCombined Law:: Example 1Example 1
• A helium filled balloon has a volume of 50.0 L at 25 ºC and 1.08 atm. What volume will it have at 0.855 atm and 10 ºC?
Given: VV11 = 50.0 L = 50.0 L
PP11 = 1.08 atm = 1.08 atm
TT11 = 25 ºC + 273 = 298 K = 25 ºC + 273 = 298 K
P P22 = 0.855 atm = 0.855 atm
TT22 = 10 ºC + 273 = 283 K = 10 ºC + 273 = 283 K
VV2=2=
Find: VV22
Combined LawCombined Law:: Example Example 22
• A sample of air has a volume of 140.0 mL at 67 ºC under 2 atm. At what temperature will its volume be 50.0 mL under 2 atm?
Given: VV11 = 140.0 L = 140.0 L
TT11 = 67 ºC + 273 = 340 K = 67 ºC + 273 = 340 K
V V22 = 50.0 mL = 50.0 mL
PP11 = P = P22
Find: TT22
BoyleBoyle’’s Laws Law:: Pressure & VolumePressure & Volume
• As pressure increases, volume decreases
↑P ↓V
↓P ↑V
P1V1 = P2V2
BoyleBoyle’’s Laws Law
• Think about why this is true:– Pressure is caused by gas molecules hitting the
container– If the volume of the container is decreased, the same
number of gas molecules are moving in a much smaller area & will hit the container more often
BoyleBoyle’’s Laws Law:: Example 1 Example 1• A sample of oxygen gas has a volume of
150 mL when its pressure is 0.947 atm. What will the volume of the gas be at a pressure of 0.987 atm?
Given: VV11 = 150 mL = 150 mL
PP11 = 0.947 atm = 0.947 atm
PP22 = 0.987 atm = 0.987 atm
Find: VV22
BoyleBoyle’’s Laws Law:: Example 1 Example 1Given: VV11 = 150 mL = 150 mL
PP11 = 0.947 atm = 0.947 atm
PP22 = 0.987 atm = 0.987 atm
Find: VV22
Plan: PP11VV11 == PP22VV22
PP11VV11== VV22
PP22Solve:
VV22 ==(0.947atm)(150 mL)(0.947atm)(150 mL)
0.987 atm0.987 atm
VV22 == 144 mL144 mL
Check: ↑P ↓V ? yes↑P ↓V ? yes
BoyleBoyle’’s Laws Law:: Example 2 Example 2• A gas has a pressure of 1.26 atm and
occupies a volume of 7.40 L. If the gas is compressed to a volume of 2.93 L, what will its pressure be?
Given: PP11 = 1.26 atm = 1.26 atm
VV11 = 7.40 L = 7.40 L
VV22 = 2.93 L = 2.93 L
Find: PP22
BoyleBoyle’’s Laws Law:: Example 2 Example 2Given: PP11 = 1.26 atm = 1.26 atm
VV11 = 7.40 L = 7.40 L
VV22 = 2.93 L = 2.93 L
Find: PP22
Plan: PP11VV11 == PP22VV22
PP11VV11== PP22
VV22Solve:
PP22 ==(1.26atm)(7.40 L)(1.26atm)(7.40 L)
2.93 L2.93 L
PP22 == 3.18 atm3.18 atm
Check: ↓V ↑P ? yes↓V ↑P ? yes
CharlesCharles’’s Laws Law:: Volume & Volume & TemperatureTemperature
• When temperature increases, volume increases
↑T ↑V
↓T ↓ V
V1=
V2
T1 T2
All temperatures must be in Kelvin!!!
CharlesCharles’’s Laws Law
• Think about why this is true:– Increase in temp. causes molecules to move faster
– Faster molecules more collisions
– More collisions more pressure inside container
– More pressure bigger volume
CharlesCharles’’s Laws Law:: Example 1Example 1
• A sample of neon gas occupies a volume of 752 mL at 25 ºC. What volume will the gas occupy at 50 ºC?
Given: VV11 = 752 mL = 752 mL
TT11 = 25 ºC + 273 = 298 K = 25 ºC + 273 = 298 K
TT22 = 50 ºC + 273 = 323 K = 50 ºC + 273 = 323 K
Find: VV22
CharlesCharles’’s Laws Law:: Example Example 11
Given: VV11 = 752 mL = 752 mL
TT11 = 25 ºC + 273 = 298 K = 25 ºC + 273 = 298 K
TT22 = 50 ºC + 273 = 323 K = 50 ºC + 273 = 323 K
Find: VV22
Plan: VV11 == VV22
TT11 TT22
VV1 1 TT22== VV22
TT11Solve:VV22 ==
(752 mL)(323 K)(752 mL)(323 K)
298 K298 K
VV22 == 815 mL815 mL
Check: ↑T ↑ V ? yes↑T ↑ V ? yes
CharlesCharles’’s Laws Law:: Example 2Example 2
• A helium balloon has a volume of 2.75 L at 20 ºC. If you bring it outside on a cold day, the volume decreases to 2.46 L. What is the outside temperature in ºC?
Given: VV11 = 2.75 L = 2.75 L
TT11 = 20 ºC + 273 = 293 K = 20 ºC + 273 = 293 K
VV22 = 2.46 L = 2.46 L
Find: TT22
CharlesCharles’’s Laws Law:: Example 2 Example 2Given: VV11 = 2.75 L = 2.75 L
TT11 = 20 ºC + 273 = 293 K = 20 ºC + 273 = 293 K
VV22 = 2.46 L = 2.46 L
Find: TT22
Plan: VV11 == VV22
TT11 TT22
VV2 2 TT11== TT22
VV11Solve:TT22 ==
(2.46 L)(293 K)(2.46 L)(293 K)
2.75 L2.75 L
TT22 == 262 K – 273 = -11 ºC 262 K – 273 = -11 ºC
Check: ↓↓ V V ↓↓ T ? yesT ? yes
Gay-LussacGay-Lussac’’s Laws Law:: Pressure & TemperaturePressure & Temperature
• When temperature increases, pressure increases
↑T ↑P
↓T ↓P
P1=
P2
T1 T2
Remember: all temperatures must
be in Kelvin!!!
Gay-LussacGay-Lussac’’s Laws Law
• Think about why this is true:– Increase in temp. causes molecules to move faster
– Faster molecules more collisions
– More collisions more pressure inside container
Gay-LussacGay-Lussac’’s Laws Law:: Example 1Example 1
• Gas in an aerosol can is at a pressure of 3.00 atm 25 ºC. What would the pressure be in the can at 52 ºC?
Given: PP11 = 3.00 atm = 3.00 atm
TT11 = 25 ºC + 273 = 298 K = 25 ºC + 273 = 298 K
TT22 = 52 ºC + 273 = 325 K = 52 ºC + 273 = 325 K
Find: PP22
Gay-LussacGay-Lussac’’s Law s Law :: Example 1Example 1
Given: PP11 = 3.00 atm = 3.00 atm
TT11 = 25 ºC + 273 = 298 K = 25 ºC + 273 = 298 K
TT22 = 52 ºC + 273 = 325 K = 52 ºC + 273 = 325 K
Find: PP22
Plan: PP11 == PP22
TT11 TT22
PP1 1 TT22== PP22
TT11Solve:PP22 ==
(3.00 atm)(325 K)(3.00 atm)(325 K)
298 K298 K
PP22 == 3.27 atm 3.27 atm
Check: ↑T ↑P ? yes↑T ↑P ? yes
Gay-LussacGay-Lussac’’s Laws Law:: Example 2Example 2
• Before you leave on a road trip, the pressure in your car tires is 1.8 atm at 20 ºC. After driving all day, the pressure gauge read 1.9 atm. What temperature (in ºC) are your tires?
Given: PP11 = 1.8 atm = 1.8 atm
TT11 = 20 ºC + 273 = 293 K = 20 ºC + 273 = 293 K
PP22 = 1.9 atm = 1.9 atm
Find: TT22
Gay-LussacGay-Lussac’’s Law s Law :: Example 2Example 2
Given: PP11 = 1.8 atm = 1.8 atm
TT11 = 20 ºC + 273 = 293 K = 20 ºC + 273 = 293 K
PP22 = 1.9 atm = 1.9 atm
Find: TT22
Plan: PP11 == PP22
TT11 TT22
PP2 2 TT11== TT22
PP11Solve:TT22 ==
(1.9 atm)(293 K)(1.9 atm)(293 K)
1.8 atm1.8 atm
TT22 == 310 K – 273 = 37 ºC 310 K – 273 = 37 ºC
Check: ↑P ↑P ↑↑ T ? yesT ? yes
Quiz Topics Next ClassQuiz Topics Next Class
1. KMT
2. Properties of Gases
3. Combined gas law calculation
4. P, V, T relationship
5. Converting Celsius to Kelvin