Term
| State Normal atmospheric pressure in five standard units |
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Definition
1 atm
760 torr
101.3 kilopascals
14.7 lbs/square inch |
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Term
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Definition
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Term
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Definition
| An instrument, invented by Torricielli in 1643, which measures atmospheric pressure. An evacuated glass tube in which a column of mercury rises or falls with changing pressure. |
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Term
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Definition
| An instrument used to measure pressure of gases in a closed container. |
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Term
| State three postulates of the Kinetic-Molecular Theory of Gases |
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Definition
1. Matter is composed of very small particles; a gas is mostly empty space.
2. Particles are in constant random motion.
3. Collisions are elastic. |
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Term
| State the formula for Graham's Law of Diffusion. |
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Definition
In a mixture of gases A, B:
(RA)(MWA)1/2 = (RB)(MWB)1/2
MW = Molecular Weight
R = Rate of diffusion |
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Term
| Do heavy or light gases diffuse faster? |
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Definition
| Light gases diffuse faster. |
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Term
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Definition
V1/T1 = V2/T2
Volume and temperature have a direct relationship when pressure and moles of gas remain constant.
V = volume
T = Kelvin |
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Term
Solve this problem:
At 300 K, a gas has a volume of 10 liters.
Find the volume at 400 K |
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Definition
Use Charles' Law: V1/T1 = V2/T2
V2 = 13.3 L |
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Term
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Definition
(P1)(V1) = (P2)(V2)
Pressure and volume have an inverse relationship when temperature and moles of gas remain constant.
P = Pressure
V = Volume |
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Term
| A sample of gas has a volume of 25 L at 800 torr. Find the volume at 400 torr. |
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Definition
Use Boyle's law: (P1)(V1) = (P2)(V2)
V2 = 50 L |
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Term
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Definition
P1V1/T1 = P2V2/T2
Moles of gas constant
P = Pressure
V = Volume
T = Kelvin |
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Term
| Dalton's Law of Partial Pressures |
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Definition
In a gas mixture, the total pressure equals the sum of the partial pressures of each component.
Ptotal = P1 + P2 + P3 ..... |
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Term
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Definition
PV = nRT
P = Pressure (atmospheres)
V = Volume (liters)
n = # of moles
R = 0.0820 (L atm)/(mol K)
T = temperature in K |
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Term
| How many moles of H2 gas are there in 20 L at 4 atm and 400K? |
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Definition
Use the Ideal Gas Law: PV = nRT
n = 2.44 moles |
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Term
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Definition
| Standard temperature (0 C, 273 K) and standard pressure (1 atm or 760 torr) |
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Term
| Gay-Lussac's Law of Combining Gas Volumes |
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Definition
| When only gases are involved in a reaction, the volumes of reactants and products are in a small, whole number ratio. |
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Term
| Avagadro's Law (for gases) |
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Definition
| Under the same conditions of temperature and pressure, equal volumes of gases contain equal numbers of moles. |
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Term
| What is the volume of 1 mole of any gas at STP? |
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Definition
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Term
N2 + 3H2 ↔2 NH3
In the above reaction, how many L of NH3 will be produced from 6 L of H2? |
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Definition
According to Gay-Lussac's Law, the volumes of gases are in direct proportion to the coefficients in the equation.
x = 4 L of ammonia |
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