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14 Cards in this Set
- Front
- Back
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How is equilibria involving gases usually expressed? |
As Kp |
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What is used instead of concentration of reactants? |
Partial pressures |
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Why can pressure be used instead? |
Pressure and concentration are proportional to one another |
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What is the expression for Kp? |
Kp= p(products)/p(reactants) |
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Which brackets are used? |
Normal, NOT SQUARE! |
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What must you ensure is the same when finding Kp? |
The units |
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What units can be used for partial pressure? |
Pa, kPa or atm |
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What is 1 atm equivalent to? |
101kPa |
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How do you work out mole fraction? |
Number of moles of A/ Total moles in mixture |
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What can be used to express the molar fraction? |
x |
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How do you work out partial pressure of a gas? |
Mole fraction x total pressure |
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What can be used to show total pressure? |
P |
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What do you do with species with states other than a gas? |
Ignore them |
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What do you do if you only have initial moles? |
Draw out the table to work out equilibrium moles, then work out molar fraction. After this you can work out partial pressure and sub this into the Kp expression to find the value of Kp. |
