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Definition
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Definition
Model of an ideal gas:
-No volume
-No forces (but repulsive due to collisions)
-Completely elastic collision
-Kinetic Energy is directly proportional to temperature |
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Definition
PV=nRT
(R=0.08206 L atm K-1mol-1 or 8.314J K-1mol-1) |
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| Volume of one mole of an ideal gas at STP |
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| Number of moles of gas a / total moles of the sample |
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| The total pressure exerted by a gaseous mixture is the sum of the partial pressures of each of its gases. |
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| Spreading of a gas from high pressure to low pressure through a pinhole. |
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Definition
| Spreading of one gas into another gas or into empty space. |
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Definition
| effusion rate1/effusion rate2 = √M2/√M1 |
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| Real gases deviate from Ideal gases at: |
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Definition
| High pressure and Low Temperature |
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| Arrhenious Equation for rate constant, k, of a reaction |
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| Sum of all the orders of each respective reactant. |
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| The rate of the slowest elementary step that determines the overall reaction. |
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| Slowest step is the first step |
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Definition
The rate law can be derived directly from this step and no other.
Ex:
1. NO2+NO2-->NO3+NO (slow)
2. NO3+CO-->NO2+CO2 (fast)
rate = k[NO2]2 |
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| Slowest step is other than the first step |
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Definition
The slow step is still rate determining but setps prior to the slow step will contribute to the rate determing step.
Ex:
1. NO+Br2-->NOBr2 (fast)
2. NOBr2+NO-->2NOBr (slow)
rate = k[NOBr2][NO] |
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Rate of the forward equals the reverse.
This is the point of greatest entropy. |
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aA+bB-->cC+dD
The Law of Mass Action |
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Definition
K=[C]c[D]d/[A]a[B]b
K is the equilibrium constant |
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Definition
Q=[C]c[D]d/[A]a[B]b
Q always changes towards K.
Q = K, Equilibrium
Q>K, leftward shift
Q<K, rightward shift |
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| Le Chatlelier's Principle |
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Definition
When a system at equilibrium is stressed, the sstem will shift in a direction to reduce the stress.
1)Adding/removing reactants/products
2)Changing the pressure in the system
3) heating/cooling |
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