equilibrium Flashcards

1
Q

a reversible reaction

A

one in which the products react to give back the reactants
the reaction goes in both directions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what is an example of an equilibrium reaction

A

production of ammonia
N2 + 3H2 = 2NH3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

chemical equilibrium

A

a state of dynamic balance in reversible reaction where the rate of the forward reaction is the same as the rate of the reverse reaction
ie the concentration remains constant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

dynamic state

A

the reactants are continuously forming products and products are continuously forming reactants

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

dynamic equilibrium

A

the rate of the forward reaction is the same as the reverse reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

why does H2 have a greater concentration than N2 in the Haber Bosch process

A

from the balanced equation the ratio is 3:1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

explain how the concentration of H2 and N2 changes throughout Haber Bosch process

A

as they react together the concentration of both decreases and the conc of ammonia increases

the conc of H2 and N2 is high at the start as they have not reacted together yet

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

what is important to remember if drawing the Haber Bosch process graph

A

at time 0 there is NO ammonia in the reaction vessel. the conc of NH3 must start at (0,0) to show this

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

describe the rate of reaction in the Haber Bosch process

A

the rate of the forward reaction decreases and the reverse increases until the rate of the forward is equal to the reverse. this is reflected by the horizontal part of the graph

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

how do we know when equilibrium has been reached

A

when the rate of reaction remains constant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

how would you describe concentration at dynamic equilibrium

A

all concentrations are constant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

why does the concentration remain constant when equilibrium is reached

A

even though the reaction is still happening, the rate of the forward and reverse reactions are the same so the relative conc of each substance is not changing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Le Chatelier’s Principle

A

if a stress is applied to a system at equilibrium the system readjusts to relieve stress applied

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

what are the 3 stresses

A

change in;
pressure
temperature
concentration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

which side does increasing temp favour

A

endothermic (+)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

which side does decreasing temp favour

A

exothermic (-)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what does increasing pressure do to equilibrium

A

shifts equilibrium to the side with the fewest number of molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what does increasing concentration do to equilibrium

A

equilibrium shifts to the other side to relieve stress

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what does decreasing concentration do to equilibrium

A

equilibrium shifts to the side that it was on to reduce stress

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what effects do catalysts have on equilibrium

A

no effect
a catalyst speeds up the rate at which a system reaches equilibrium
they affect both sides of the equation equally so it has no effect on equilibrium position

21
Q

how to answer a conc q

A

state which way equilibrium will shift and why:
if more of y is added
equilibrium will shift to the right to relieve stress
more x is produced

if y is removed
equilibrium will shift to the left to relieve stress
yield of x is reduced

22
Q

how do we read an equilibrium equation in terms of temperature

A

read from left to right
the arrow pointing towards the delta H shows which reaction relates to the temperature ie if the forward reaction is endo or exo

be careful because they have changed the direction of the arrows before in the exam

23
Q

how to answer a q on temp

A

identify which of the reactions is endo or exo
state which way equilibrium will shift and why

increasing temperature will force the equilibrium to shift in the endothermic direction to relieve stress ie to the L/R
thus the yield of x will decrease

decreasing temp will force equilibrium to shift in the exothermic direction to relieve stress ie to the L/R
thus the yield of x will increase

24
Q

what state does pressure affect

A

REAGENTS HAVE TO BE GASES

25
what effect does increasing pressure have on equilibrium
in all GASEOUS reactions it will force equilibrium to shift to the side that decreases volume ie the side with the fewest no of molecules
26
what effect does pressure have on a reaction happening in an aqueous solution
no effect as liquid cannot be compressed
27
temp of the formation of ammonia
500 degrees C
28
pressure of the formation of ammonia
200 atm
29
catalyst of of the formation of ammonia
iron
30
why do we not use a lower temperature when forming ammonia
decreasing temperature forces the reaction in the exothermic direction so more ammonia will be produced however at lower temperatures the colliding particles have much less kinetic energy so there are fewer effective collisions this means that the rate of the production of ammonia is very slow at low temp which is actually very expensive thus less profit.
31
what is a compromise temperature in relation to the manufacturing of ammonia
the temperature is low enough to give an acceptable yield of ammonia but high enough to guarantee an acceptable rate of ammonia formation
32
is the production of ammonia endo or exo
exo ie more forms at lower temp
33
temperature of the manufacture of sulphuric acid
450 C
34
pressure of the manufacture of sulphuric acid
just above atmospheric pressure
35
catalyst of the manufacture of sulphuric acid
vanadium pentoxide, V2O5
36
what is the contact process
used to manufacture sulphuric acid SO2 reacts with oxygen gas over a catalyst
37
how is SO2 obtained for the contact process
by burning sulphur in air
38
what is another catalyst that can be used in the contact process
platinum
39
why is platinum not used as a catalyst in the contact process
it is easily poisoned by impurities in the reaction
40
how is sulphuric acid manufactured from the contact process
SO3 formed in the reaction is dissolved in rainwater to form sulphuric acid SO3 + H2O ---> H2SO4
41
what is the balanced equation for the contact process
2SO2(g) + O2(g) ----> 2SO3(g)
42
what is the equilibrium constant
Kc
43
what is Kc used for
to describe the relationship between the reactants and products
44
what is the only stress that effects Kc
TEMPERATURE
45
how do you write KC
aA + bB --> cC + dD Kc = top line: [C] to the power of c x [D] to the power of d bottom line: [A] to the power of a x [B] to the power of b RIGHT SIDE ALWAYS ON TOP SQUARE BRACKETS ONLY
46
what do the square brackets represent in the Kc expression
mol/L
47
how does changing temperature affect Kc
if equilibrium shifts to the left the value for Kc decreases if it shifts to the right the value for Kc increases
48
why does pressure not affect Kc
it changes the no of molecules but the change in volume balances this out in the calculation thus Kc is not affected