ideal gas law. 1. avogadro’s principle how much volume will one mole of hydrogen, oxygen, and...
TRANSCRIPT
![Page 1: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/1.jpg)
Ideal Gas Law
![Page 2: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/2.jpg)
1. Avogadro’s Principle
How much volume will one mole of hydrogen, oxygen, and helium occupy at STP?
Using the molar mass and gas density at STP :
H2 : H2
O2 : O2
He : He
2x16.0g1mole
cm3
0.001429gmLcm3
L1000mL 22.4L
mole
2x1.00794g1mole
cm3
0.0000899gmLcm3
L1000mL 22.4L
mole
1x4.0g1mole
cm3
0.00017847gmLcm3
L1000mL 22.4L
mole
![Page 3: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/3.jpg)
It appears that :1 mole of a gas, at STP occupies 22.4 LSTP – standard temperature and pressureSTP - 0ºC, 101.3 kPa (1 atm, 760 mmHg)6.02 x 1023 gas particles, at STP, 22.4 L
Avogadro’s Principle – At equal temperature and pressure, equal volumes of gases contain equal number of molecules.
= constant V = volume, n = molesn
V
![Page 4: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/4.jpg)
![Page 5: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/5.jpg)
Moles ↑ Volume ↑ Direct Relationship Moles ↓ Volume ↓ A relationship between the number of particles
and the volume NOT a relationship between mass and volume!
H2 1 mole 2.016 g 22.4 L 0°C, 1 Atm
O2 1 mole 32.0 g 22.4 L 0°C, 1 Atm
He 1 mole 4.0 g 22.4 L 0°C, 1 Atm
DifferentGases
Same Numberof particles
DifferentMasses
SameVolume
Same Temperature
Pressure
![Page 6: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/6.jpg)
Molar Volume – the volume of 1 mole of a gas, at a specified temperature and pressure.
Molar volume at STP, is 22.4 liters.
1 mole H2, at STP, occupies 22.4 L
1 mole O2, at STP, occupies 22.4 L
1 mole CO2, at STP, occupies 22.4 L
![Page 7: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/7.jpg)
2. Ideal Gas Law Avogadro’s Principle : = constant
V = volume n = moles
Combined Gas Law :
Ideal Gas Law :
or PV = nRT Where R = Ideal Gas Constant
constantT
PV
constantTn
PV
n
V
![Page 8: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/8.jpg)
![Page 9: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/9.jpg)
![Page 10: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/10.jpg)
PV = nRTP = pressure, kilopascals, kPaV = volume, Liters, Ln = number of moles
(convert grams to moles using Molar Mass)T = temperature, kelvin, K
R = Ideal Gas Constant,
Convert all units to the above, and you will only have to memorize one ideal gas constant!
Kmole
LkPa8.314
![Page 11: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/11.jpg)
![Page 12: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/12.jpg)
Calculate the ideal gas constant for STP, 1 mole of gas, and 22.4 liters!
PV=nRT (101.3 kPa)(22.4L) = (1mole)(R)(273K)
= R
R =
3K)(1mole)(27
(22.4L)(101.3kPa)
Kmole
LkPa8.314
![Page 13: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/13.jpg)
3. Ideal and Real Gases
![Page 14: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/14.jpg)
What volume does 3.5 moles of nitrogen gas occupy at STP?
![Page 15: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/15.jpg)
How many grams of hydrogen gas are in 9.0 L at STP?
![Page 16: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/16.jpg)
What volume will 125 g of carbon dioxide occupy at STP?
![Page 17: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/17.jpg)
What is the volume (in liters) of 2.00 g CS2 vapor at 276 mm Hg and 70°C?
![Page 18: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/18.jpg)
How many grams are in a sample of ammonia gas at 786 mm Hg, 2.5 L, and 28°C?
![Page 19: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/19.jpg)
What pressure, in kPa, is exerted by 1.75 g of hydrogen gas in a 4.08 liter container at 35°C?
![Page 20: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/20.jpg)
What is the volume of a gas that is 0.023 mole of nitrogen gas at STP?
![Page 21: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/21.jpg)
How many moles of air are in a 6.0 L tire at STP?
![Page 22: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/22.jpg)
How many moles of oxygen are in a 5.5 L canister at STP?
![Page 23: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/23.jpg)
What mass of helium is in a 2.00 L balloon at STP?
![Page 24: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/24.jpg)
Calculate the number of moles of gas that occupy a 3.45 L container at a pressure of 150 kPa and a temperature of 45.6°C.
![Page 25: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/25.jpg)
What is the pressure in mmHg that a 0.44 g sample of carbon dioxide gas will exert at a temperature of 46.2°C when it occupies a volume of 5.00 L?
![Page 26: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/26.jpg)
Calculate the mass of oxygen gas present in a 2.50 L sample kept at 1.66 atm pressure and a temperature of 10.0°C.
![Page 27: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/27.jpg)
5. Density of a Gas Density = PV = nRT
so Density =
volumemass
Vn
RTP
volumemoles
Vn
Litersgrams
molegrams
xLitersmoles
MassMolarxRTP
![Page 28: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/28.jpg)
What is the density of ammonia gas if the pressure is 700.0 mmHg and the temperature is 63.0°C?
![Page 29: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/29.jpg)
What is the density of sulfur dioxide at STP?
![Page 30: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/30.jpg)
What is the density of carbon dioxide at 26.0°C and 1.15 atm?
![Page 31: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/31.jpg)
6. Molar Mass of Gases Molar mass =
Used to identify a gas. PV=nRT Solve for moles (n) from given pressure, volume,
and temperature. Divide given grams by calculated moles (n).
molegrams
![Page 32: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/32.jpg)
What is the molar mass of a 1.25 g sample of gas with a volume of 1.00 L, at 730.0 mmHg, and 27.0°C?
![Page 33: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/33.jpg)
What is the molar mass of 0.427 g of a gas that occupies 125 mL at STP?
![Page 34: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/34.jpg)
What is the molar mass of a sample of gas that has a density of 0.285 g/L at 101 kPa and 29°C?
![Page 35: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/35.jpg)
What is the molar mass of a gas if 142 g of the gas occupies a volume of 45.1 L at 28.4°C and 94.6 kPa?
![Page 36: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/36.jpg)
7. Gas Stoichiometry
2 H2(g) + O2(g) 2 H2O(g)
2 molecules H2 + 1 molecule O2 2 molecules H2O
2 moles H2 + 1 mole O2 2 moles H2O at STP 2(22.4 L) H2 + 1(22.4 L) O2 2 (22.4 L) H2O
2 volumes H2 + 1 volume O2 2 volumes H2O At constant pressure and temperature, the
volumes of gaseous reactants and gaseous products can be expressed as ratios of small whole numbers.
![Page 37: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/37.jpg)
At constant pressure and temperature, the mole ratio is equal to the volume ratio.
Calculating volumes of gases in chemical reactions:
1. Write a balanced chemical equation.
2. If the temperature and pressure remains constant during the chemical reaction, use the volume ratio.
3. Remember at STP, 1 mole of any gas occupies 22.4L.
![Page 38: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/38.jpg)
If you are dealing with chemical reactions where:
Mixture of solids, liquids, and gases Change in temperature and/or pressure for
gases You will have to use the Ideal Gas Law.
1. Write a balanced chemical equation.
2. Calculate moles of gas from PV=nRT
3. Use mole ratio.
4. Convert moles of product to volume using PV=nRT.
![Page 39: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/39.jpg)
Reactant A(gas) + B Product C + Product D(solid)
gas = P, V, T
moles A
PV=nRT
mass, grams
MM D
AmolesDmoles
moles D
![Page 40: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/40.jpg)
Reactant A(gas) + B Product C(solid) + Product D(gas)
gas = P, V, T
moles A
PV=nRT
gas, P, V, T
PV=nRT
AmolesDmoles
moles D
![Page 41: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/41.jpg)
If I have 27.0 L of hydrogen gas that reacts with an excess amount of nitrogen gas, how many liters of ammonia will be produced at the same temperature and pressure?
![Page 42: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/42.jpg)
How many liters of carbon monoxide, at 27.0°C and 25.0 kPa can be produced from burning 65.5 g of carbon?
![Page 43: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/43.jpg)
What volume of oxygen can be collected at 100.0 kPa and 25°C when 30.6 g KClO3 decomposes?
![Page 44: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/44.jpg)
What volume of bromine gas (at 0.00°C, 98.0 kPa) is produced when 95.0 L of chlorine (at 50.0°C, 50.5 kPa) react with excess HBr?
![Page 45: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/45.jpg)
Calculate the mass of hydrogen peroxide needed to obtain 0.460 L of oxygen gas at STP.
![Page 46: Ideal Gas Law. 1. Avogadro’s Principle How much volume will one mole of hydrogen, oxygen, and helium occupy at STP? Using the molar mass and gas density](https://reader033.vdocuments.mx/reader033/viewer/2022061507/5697bff81a28abf838cbf537/html5/thumbnails/46.jpg)
Magnesium metal will “burn” in carbon dioxide to produce elemental carbon and magnesium oxide. What mass of magnesium will “burn” in a 255 mL container of CO2 at 77.0°C and 65.0 kPa?