1.6 equilibria and redox reactions Flashcards

1
Q

what is dynamic equilibrium?
when does it occur?

A

when the forward and backward rate are equal and the conc of reactants and products isn’t changing.
closed system at constant temp

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2
Q

what is Le Chatelier’s principle?

A

if a reaction at equilibrium is subjected to a change in conc, pressure or temp, position of equilibrium shifts to counteract the change.

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3
Q

what happens if you increase the conc of a reactant in a reaction at equilibrium?

A

equilibrium tries to get rid of the extra reactant by making more product so equilibrium shifts right. vice versa for increasing conc of product or for decreasing them.

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4
Q

what happens if you increase the pressure of a reaction at equilibrium?

A

only affects equilibria including gases
equilibrium shifts to side with fewer gas molecules to reduce the pressure. vice versa for decreasing pressure

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5
Q

what happens if you increase the temperature of a reaction at equilibrium?

A

equilibrium shifts in endothermic direction (positive delta H) to absorb this heat. vice versa for decreasing temp (moves in exo direction to replace heat.

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6
Q

example of reversible reactions

A

page 127 and 128 of text book

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7
Q

what are the conditions of making ethanol from ethene and steam? why are they like this?

A

high pressure so forward reaction is favored (less molecules on left) but expensive so 60 atm is a compromise of max yield and min cost
low temp as forward is exo and lower temp shifts it in exo direction but that means slow ror so 300 as compromise of yield and ror
phosphoric acid catalyst
small bit of ethene reacts each time so reused

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8
Q

conditions of making methanol from carbon monoxide and hydrogen
why?

A

50-100 atm
250 degrees c
catalyst of mixture of copper, zinc oxide, aluminium oxide
compromise between high yield and low cost

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9
Q

What is Kc? what is the equation of the reaction and Kc?

A

the equilibrium constant (at that specific temp)
it is a ratio worked out from all concs of reactants and products once equilibrium is reached
aA + bB = dD + eE (reversible arrow)
Kc = [D]^d x [E]^e / [A]^a x [B]^b

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10
Q

what does [A] mean?
what does a mean?

A

the conc of A in moldm-3
the number of moles of a

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11
Q

how to find equilibrium conc?

A

ICE method
initial moles, change in moles, end moles (at equilibrium) (use ratio to work out change in moles)
divide all end moles by volume to find conc

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12
Q

why might is not matter if you arent given volume in Kc question?

A

if there are no units then the volumes would all cancel in the equation for Kc

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13
Q

how to find units for Kc?

A

put units into Kc instead of numbers and simplify

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14
Q

how can you find equilibrium conc from Kc?

A

put all values in and rearrange to solve

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15
Q

what factors affect equilibrium position?

A

concentration, pressure, temperature

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16
Q

why does a catalyst not affect the equilibrium position?

A

it increases the rate of the forward and backward reactions by the same amount

17
Q

does temperature affect value of Kc?

A

yes.
if the change results in more product formed, Kc will rise
if it means less product is formed, Kc will fall
this is why Kc is at a given temperature

18
Q

does concentration affect value of Kc?

A

no

19
Q

does pressure affect value of Kc?

A

no

20
Q

does adding a catalyst affect value of Kc?

A

no

21
Q

what is a redox reaction?

A

reduction and oxidation happen simultaniously

22
Q

what is an oxidising agent?
what is a reducing agent?

A

oxidising- accepts electrons and gets reduced
reducing- donates electrons and gets oxidised

23
Q

what is the oxidation state of an element?

A

total number of electrons an element has donated or accepted

24
Q

what is the oxidation state of uncombined elements and elements bonded to just an identical atom?

A

0

25
Q

what is the oxidation state of a monoatomic ion?

A

the same as its charge

26
Q

what is the oxidation state of compounds or compound ions?

A

the sum of oxidation states of all the atoms- also equal to the charge of the compound

27
Q

what are the oxidation states usually of the following/ what are the exceptions?
group 1 metals
group 2 metals
flourine
(hydrogen, oxygen, chlorine and exeptions)

A

group 1 metals- +1
group 2 metals- +2
flourine- -1
hydrogen +1 unless in metal hydrides
oxygen -2 unless in peroxides/ compounds with F
chlorine -1 unless in compounds with O or F

28
Q

how do you find oxidation state from systematic names?

A

shown as roman numerals in brackets following element they correspond with eg iron(II) sulphate and iron (III) sulphate

29
Q

what is a half equation?

A

equation showing electrons to balance charges

30
Q

what is a redox equation?

A

equation showing oxidation and reduction

31
Q

how do you work out redox equations?

A

combine the oxidation and reduction half equations making sure they both have same number of electrons (can multiply whole equation by a common factor) then cancel out electrons

32
Q

how to write half equations

A

check if element being oxidised is balanced
add water molecules to balance oxygen atoms in the equation
add hydrogen ions to balance the hydrogen atoms in the equation
add electrons to conserve the charge
use oxidation states/ gain or loss of electrons to see if oxidation/ reduction occured