topic 11: equilibrium II

Question 1

what is the dynamic equilibrium

Answer 1

when forward and backward reactions are occurring at equal rates. the concentrations of reactants and products stays constant and the reaction is continuous

Question 2

what is the general formula of Kc (use the equation
mA + nB —> pC + qD

Answer 2

[ C]p [D]q
- m,n,p,q are the stoichiometric balancing numbers
- A,B,C,D stand for the chemical formula

Question 3

what is the Kc

Answer 3

equilibrium constant

Question 4

what is the unit used in Kc for the concentration

Answer 4

mol dm-3

Question 5

what is the equation to work out the moles of reactants at equilibrium

Answer 5

moles of reactant at equilibrium = initial moles – moles reacted

Question 6

what is the equation to work out the moles of products at equilibrium

Answer 6

moles of product at equilibrium = initial moles + moles formed

Question 7

CH3CO2H +CH3CH2OH <—-> CH3CO2CH2CH3 + H2O
PRACTICAL: part 1 - preparing the equilibrium mixture

Answer 7

1. use burettes to prepare a mixture in boiling tube of carboxylic acid, alcohol, and dilute sulfuric acid
2. swirl and bung tube. leave the mixture to reach equilibrium for one week

Question 8

CH3CO2H +CH3CH2OH <—-> CH3CO2CH2CH3 + H2O
PRACTICAL: part 2 - titrating the equilibrium mixture

Answer 8

1. rinse a 250 cm3 volumetric flask with distilled water. use a funnel to transfer the contents of the boiling tube into the flask. rinse the boiling tube with water and add the washings to the volumetric flask
2. use distilled water to make up the solution in the volumetric flask to exactly 250 cm3. stopper the flask, then invert and shake the contents thoroughly
3. use the pipette to transfer 25.0 cm3 of the diluted equilibrium mixture to a 250 cm3 conical flask
4. add 3 or 4 drops of phenolphthalein indicator to the conical flask
5. set up the burette with sodium hydroxide solution
6. add the sodium hydroxide solution from the burette until the mixture in the conical flask just turns pink. record this burette reading in your table
7. repeat the titration until you obtain a minimum of two concordant titres

Question 9

PRACTICAL: why does the pink colour of the phenolphthalein in the titration fade after the end-point of the titration has
been reached

Answer 9

because the addition of sodium hydroxide may make the equilibrium shift towards the
reactants

Question 10

PRACTICAL: what does the sodium hydroxide react with

Answer 10

the sulfuric acid catalyst and any unreacted carboxylic acid in the equilibrium mixture

Question 11

what is the partial pressure of a gas in a mixture

Answer 11

the pressure that the gas would have if it alone occupied the volume
occupied by the whole mixture

Question 12

how do you work out the mole fraction of a gas

Answer 12

number of moles of a gas/ total number of moles of all gases

Question 13

who do you work out the partial pressure of 1 gas

Answer 13

= mole fraction x total pressure

Question 14

what is the unit of pressure

Answer 14

atm

Question 15

work out the expression of Kp for the equation
N2(g) + 3H2(g) <—> 2 NH3(g)

Answer 15

p(N2) p(H2)^3

Question 16

the substances in what state should be included in the Kp expression

Answer 16

only gases

Question 17

what is the Kc value if the reaction doesn’t happen

Answer 17

Kc < 10^-10

Question 18

what is the Kc value if reactants are predominate in an equilibrium

Answer 18

Kc is approximately 0.1

Question 19

what is the Kc value when equal amounts of reactants and products

Answer 19

Kc = 1

Question 20

what is the Kc value when products are predominate in equilibrium

Answer 20

Kc is approximately 10

Question 21

what is the Kc value when the reaction goes too completion

Answer 21

Kc > 10^10

Question 22

as ΔStotal increases,, what happens to the equilibrium constant

Answer 22

increases

Question 23

what is the equation of ΔS

Answer 23

ΔS = R lnK

Question 24

what is the effect of temperature on position of equilibrium and Kp

Answer 24

Both the position of equilibrium and the value of Kc or Kp will change it temperature is altered
- if temperature is increased the reaction will shift to oppose the change and move in the backwards endothermic direction
- the position of equilibrium shifts left
- the value of Kc gets smaller as there are fewer products

Question 25

what is the effect of concentration on position of equilibrium and Kc

Answer 25

changing concentration would shift the position of equilibrium but the value of Kc would not change - increasing concentration of H2 would move equilibrium to the right lowering concentration of H2 and Cl2 and increasing concentration of HCl - the new concentrations would restore the equilibrium to the same value of Kc

Question 26

what is the effect of concentration and pressure on rate

Answer 26

at higher concentrations and pressures, there are more particles per unit volume and so the particles collide with a greater frequency and there will be a higher frequency of effective collisions

Question 27

why does increasing pressure not change Kp

Answer 27

- the increased pressure increases the pressure terms on bottom of Kp expression more than the top - the system is now no longer in equilibrium so the equilibrium shifts to the right, increasing mole fractions of products and decreases the mole fractions of reactants - the top of the Kp expression therefore increases and the bottom decreases until the original value of Kp is restored

Question 28

what is the effect of pressure on the position of equilibrium

Answer 28

if pressure is increased the reaction will shift to oppose the change and move in the forward direction to the side with fewer moles of gas - the position of equilibrium shifts right - the value of Kp stays the same though as only temperature changes the value of Kp

Question 29

what will happen to the Kp value if pressure is altered

Answer 29

Kp stays constant

Question 30

what is the effect of catalyst on the equilibrium constant

Answer 30

a catalyst has no effect on the position of equilibrium or values of Kc and Kp but it will speed up the rate at which the equilibrium is achieved it does not effect the position of equilibrium because it speeds up the rates of the forward and backward reactions by the same amount

Question 31

what is the effect of catalysts on the position of equilibrium

Answer 31

catalysts speeds up the rate allowing lower temperatures to be used (and hence lower energy costs) but have no effect on equilibrium

Question 32

describe the haber process

Answer 32

N2 + 3H2 <---> 2NH3 exothermic T= 450oC,P= 200 - 1000 atm, catalyst = iron low temp gives good yield but slow rate: compromise temp used high pressure gives good yield and high rate: too high a pressure would lead to too high energy costs for pumps to produce the pressure

Question 33

describe contact process

Answer 33

stage 1: S(s) + O2(g) <---> SO2(g) stage 2: SO2(g) + ½O2 (g) <---> SO3 (g) H = -98 kJ mol-1 T= 450oC, P= 1 to 2 atm, catalyst = V2O5 low temp gives good yield but slow rate: compromise moderate temp used high pressure gives slightly better yield and high rate: too high a pressure would lead to too high energy costs for pumps to produce the pressure

Question 34

what does high pressure lead to

Answer 34

high energy costs for pumps to produce the pressure and too high equipment costs to have equipment that can withstand high pressures

Question 35

what does recycling unreacted reactants do

Answer 35

recycling unreacted reactants back into the reactor can improve the overall yields of all these processes and improve their atom economy - industrial processes cannot be in equilibrium since the products are removed as they are formed to improve conversion of reactants - they are not closed systems