3.1.10 Equilibrium constant Kp for homogeneous systems Flashcards
1
Q
bracket type in kp
A
must be round brackets NOT square brackets
2
Q
how to write a Kp
A
p(products)power c
/
p (reactant)
- put a p at front as the partial pressure
- use round brackets
- otherwise like kc
3
Q
working out the units
A
- like Kc
- MUST USE THE UNITS PROVIDED IN QUESTION
4
Q
when do you not have to calculate kp
A
- If there us the same number of mols on each side of the eqm – side no need to calculate partial pressure
5
Q
how to calculate partial pressure
A
- mols ( may have to be from an ICE table)
- total mols
- molar ration
- multiply the molar ration against total pressure
6
Q
why catcalysts dont effect the kp
A
- Catalsyt effects the rate of the forward reaction and backwards reaction evenly – meaning no change to kp
7
Q
change in partial presssure of one substance in equation point
A
- Can effect partial pressure of other substances – when the partial pressure of one other substance is increased/ decreased
8
Q
calculauting a new kp rule
A
- Calculating a new kp – when mols of reactant is halved – ( original kp is square rooted (as power stuff))
9
Q
le chatiliers wording
A
- Le chatiliers principle – shifts in the …… direction. To reduce the temperature increase / to oppose the ….. in temperature.
10
Q
kp and pressure
A
- Kp is independent of pressure
11
Q
sum enthalpy change
A
- Sum enthalpy change = sum products – sum reactants ( broken – formed)
12
Q
– why value of ans and data book differ
A
- Mean bon enthalpy is not the same as actual bond enthalpy – why value of ans and data book differ
13
Q
- Environmental factor
A
think CO2 or biproducts
14
Q
what do impurities do to a catalyst
A
- Impurities block the ACTIVE SITE of the catalyst
15
Q
important point when la chitelliers and pressure
A
state how many mols on each side
