GASES. Gases The physical state of gases is defined by several physical properties Volume …
Properties of all gases
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Transcript of Properties of all gases
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Properties of all gases
Chapter 14
with Ch 13 review.
WOD are underlined.
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Properties of all gases• When working with gases, there are 4 properties that must
be considered:
Gas Properties: Mass, Volume, Pressure, Temperature
• There are multiple equations: The properties that change determine the equation to select to solve for the unknown.
• All the remaining properties must be held constant.
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From Chapter 13
Phases
• Two of the properties determine the phase of an element:
• Pressure
• Temperature
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From Chapter 13
Phases
• What happens when you increase pressure (a lot) on gas?
(What is one exception?)
• What happens when you increase temperature (a lot) on a solid?
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There is a pan of ice on the stove.
What does this Temperature graph
look like?
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WRONG!
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Properties of all gasesKNOW ALL THE FOLLOWING:
• Pressure at STP is:– 1 atm = 760 mm Hg = 101.3 kPa = 14.7 lbs/in2
• Volume– 1 mL = 0.001L = 1cm3
• Temperature at STP is 273 K (0° Celsius)– Use Kelvin (not Celsius)
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Standard Temperature and Pressure:STP, Temperature and Pressure at Sea Level
on a freezing day = 101.3 kPa, 273 K
KNOW ALL THE FOLLOWING:• Pressure at STP is:
– 1 atm = 760 mm Hg = 101.3 kPa = 14.7 lbs/in2
• Volume– 1 mL = 0.001L = 1cm3
• Temperature at STP is 273 K (0° Celsius)– Use Kelvin (not Celsius)
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Properties of all gases
• Pressure– 1 atm = 760 mm Hg = 101.3 kPa = 14.7 lbs/in2
Discuss Gage pressure in a factory (diff from atm. Vs gage pressure in a lab (Boyles Law)
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Boyle’s Law – what happens to pressure?
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Boyle’s Law P1V1 = P2V2
(mass and temperature constant) Volume of a gas varies inversely
with pressure V↑P↓ or P↑V↓P1V1 = P2V2
Or PV = Constant
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Steps to Solve Problems:1. Known: Find the knowns.
2. Unknown: Find the unknowns.3. Equation: Pick the equation that matches the knowns and unknowns.
4. Units: Make sure units are the same on both sides. T in Kelvin.
5. SigFig: Change the answer to the correct number of significant
figures.
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A 220mL balloon of air is at a pressure of 506.5kPa. What will be the volume of the balloon at
sea level (STP)?
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A 455mL balloon is taken from sea level up to a point where the
pressure is unknown. The balloon has a new volume of 1.25L. What
is the pressure?
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Review the last 2 slides. As height goes up:
What happens to pressure?What happens to volume?
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NaHCO3 + HC2H3O2 H2O +NaC2H3O2 + CO2
At STP, 2.5g of NaHCO3 produced 560 mL of CO2 gas. What would the volume of this
gas be on top of mountain where the pressure is only 250 mm Hg?
Extra credit – What is the percent yield of CO2 produced? (Use Mass ratio’s)
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NaHCO3 + HC2H3O2 H2O +NaC2H3O2 + CO2
At STP, 2.5g of NaHCO3 yields 560 mL of CO2 P2 = 250 mm Hg?
Extra credit – What is the percent yield of CO2 produced?
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Charles’s Law – What happens to a gas if it is heated?
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Charles’s Law V1/T1=V2/T2
(mass and pressure constant)
Volume of a gas varies directly with its Kelvin temperature
T↑ V↑ or T↓V↓V1/T1=V2/T2
or V/T = Constant
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A balloon is filled with 5.00L of air with a temperature of 00C.
The balloon is placed by a furnace and expands to 7.00L. What is the temperature next to
the furnace? Hint: Use 273K
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Gay-Lussac’s Law P1/T1=P2/T2
(mass and volume constant) pressure of a gas varies directly with
its Kelvin temperature P↑ T↑ or P↓T↓
P1/T1=P2/T2
or P/T=Constant
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Combined Gas Law:(Temp is in Kelvin)
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The volume of a “Get Well Soon” balloon is 2.5L at STP conditions. What would the volume of the balloon be on the moon (-930C, 1.1x10-8kPa)
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Quiz 14.2A can of compressed air ruptures
at an internal pressure of 225 lbs/in2. At standard temperature
(0.00oC) the pressure is 55.5 lbs/in2. At what temperature will the can burst (reach it bursting
pressure)?
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Ideal Gas LawPV=nRT
Prairie Village is not a Real Town R= 8.31 ( L•kPa)/(K •mol)
P, V, Tn = moles
R= 8.31 ( L•kPa)/(K •mol)
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How many grams of He are needed to fill a weather balloon that is 2520L at
sea level and 5.75oC?
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What is the pressure on the inside of a CO2 cartridge?
(There are 12.1 grams, the temperature in the room is 68.7F, and the volume is 15.9mL.)
Would the pressure change if the room temperature changed?
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PV=nRTX (0.0159L) = 0.275mol (8.31 L .kPa/mol.K) 293.4K
42,200 kPa or 42,169.33019 kPaabout 417atm
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Sample Problem
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NaHCO3 + HC2H3O2 H2O +NaC2H3O2 + CO2
A classroom has a temperature of 303K and a pressure of 105kPa. What volume of CO2 will be produced from
12.5g of NaHCO3?
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Quiz 14.3 How many moles of H2 are needed to
fill a balloon that is 2.50L, at sea level, and 295.75K?
Extra credit –H2O + Na NaOH + H2
How many grams of Na will it take to fill the balloon?
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Review
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Properties of all gases• When working with gases, there are 4 properties that must
be considered:
Gas Properties: Mass, Volume, Pressure, Temperature
• There are multiple equations: The properties that change determine the equation to select to solve for the unknown.
• All the remaining properties must be held constant.
![Page 36: Properties of all gases](https://reader036.fdocuments.us/reader036/viewer/2022062519/56814cf3550346895db9f7b2/html5/thumbnails/36.jpg)
Properties of all gasesKNOW ALL THE FOLLOWING:
• Pressure at STP is:– 1 atm = 760 mm Hg = 101.3 kPa = 14.7 lbs/in2
• Volume– 1 mL = 0.001L = 1cm3
• Temperature at STP is 273 K (0° Celsius)– Use Kelvin (not Celsius)
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Combined Gas Law:(Temp is in Kelvin)
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Ideal Gas LawPV=nRT
Prairie Village is not a Real Town R= 8.31 ( L•kPa)/(K •mol)
P, V, Tn = moles
R= 8.31 ( L•kPa)/(K •mol)
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Steps:1. Known: Find the knowns.
2. Unknown: Find the unknowns.3. Equation: Pick the equation that matches the knowns and unknowns.
4. Units: Make sure units are the same on both sides. T in Kelvin.
5. SigFig: Change the answer to the correct number of significant
figures.