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A Level Chemistry > Chemical Industry > Flashcards

Chemical Industry Flashcards

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1
Q

how can you follow rate of reaction?

A

ph
gas vol
loss of mass
colour change
titration

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2
Q

initial rate =

A

amount of reactant used or formed / time

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3
Q

how do you do the initial rate method?

A

time how long it takes for specific vol of gas to form then repeat using different concentrations of one reactant

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4
Q

iodine clock reaction equation is…

A

H2O2 + 2I- + 2H+ —> 2H2O + I2

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5
Q

what is the rate equation?

A

rate = k [A]^m x [B]^n

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6
Q

the bigger the rate constant…

A

the faster the reaction

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7
Q

how does a zero order reactant affect rate?

A

changing concentration has no effect on rate

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8
Q

how does a first order reactant affect rate?

A

if the concentration increases, rate increases proportionally

e.g. if conc doubles, rate doubles

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9
Q

how does a second order reactant affect rate?

A

if the concentration increases, rate increases proportionally squared

e.g. if conc doubles, rate quadruples

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10
Q

what is half life?

A

the half life of a reaction is the time it takes for half the reactant to be used up

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11
Q

as a reaction goes on the half life of a zero order reactant…

A

decreases as the reaction goes on

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12
Q

as a reaction goes on the half life of a first order reactant…

A

remains constant

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13
Q

as a reaction goes on the half life of a second order reactant…

A

increases as it goes on

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14
Q

you can find rate constant from….

A

half life and first order

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15
Q

does changing temperature affect rate constant?

A

yes

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16
Q

a calculated rate constant is only valid at…

A

a certain temperature

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17
Q

at a higher temperature rate constant…

A

will be higher

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18
Q

the arrhenius equation links…

A

rate constant and activation energy

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19
Q

what is the arrhenius equation?

A

k = (-Ea)/RT

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20
Q

what is the equation for equilibrium constant?

aA + bB —> dD + eE

A

Kc = [D]^d x [E]^e / [A]^a x [B]^b

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21
Q

if temperature is increased @ equilibrium

A

eqm shifts in the endothermic direction

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22
Q

if temperature is decreased @ equilibrium

A

eqm shifts in exothermic direction

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23
Q

if the increase in temperature means product yield increases…

A

Kc will increase

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24
Q

if the increase in temperature means product yield decreases…

A

Kc will decrease

25
Q

do pressure changes affect Kc?

A

no

26
Q

do catalysts have affect on Kc?

A

no

27
Q

colorimetry and ph readings can be used to…

A

find equilibrium concentrations

28
Q

what kind of molecule is a nitrogen?

A

diatomic molecule

29
Q

how many electrons are in nitrogen’s outer shell?

A

5

30
Q

what is the electron configuration of nitrogen?

A

1s2 2s2 2p3

31
Q

how do N atoms get a full shell?

A

they pair up and share 3 pairs of electrons between them

32
Q

nitrogen atoms pair up and share..

A

3 pairs of electrons between them

33
Q

nitrogen atoms pair up to form a…

A

triple bond

34
Q

why is nitrogen unreactive

A

contains a triple bond that is hard to break

35
Q

nitrogen forms three oxides that are…

A
  1. NO
  2. N2O
  3. NO2
36
Q

NO is called…

A

nitrogen monoxide

37
Q

NO (nitrogen monoxide) is a _____ gas

A

colourless

38
Q

N2O is called….

A

nitrous oxide

39
Q

nitrous oxide smells….

A

sweet

40
Q

nitrous oxide is a _____ gas

A

colourless

41
Q

NO2 is called…

A

nitrogen dioxide

42
Q

NO2 (nitrogen dioxide) is ____ and ____

A

brown and toxic

43
Q

NO2 (nitrogen dioxide) has a ___ ____

A

sharp odour

44
Q

ammonias formula is…

A

NH3

45
Q

N atoms form _____ bonds by sharing _ electron with each ____ . Leaving a ____ ____ on the nitrogen.

A
  1. covalent
  2. one
  3. hydrogen
  4. lone pair
46
Q

why is ammomia soluble in water?

A

it can form hydrogen bonds with water

47
Q

why can ammonia form dative covalent bonds?

A

it has a lone pair of electrons

48
Q

the lone pair on the ammonia allows it to act as a…

A

base

49
Q

what is the test for NH4+ ions?

A
  1. add NaOH to solution and heat
  2. if present they react with OH- ions and NH3 is produced
  3. red litmus turns blue
50
Q

nitrates react with ammonia in the presence of…

A

alkali

51
Q

the formula for nitrate ions is

A

NO3-

52
Q

how do you test for nitrate (v) ions?

A
  1. warm solution with NaOH and aluminium foil (or Devarda’s alloy)
  2. if present ammonia gas will be produced
  3. so damp red litmus turns blue
53
Q

which oxide containing nitrogen is brown and toxic?

A

nitrogen dioxide (NO2)

54
Q

which oxide containing nitrogen has a sharp odour?

A

nitrogen dioxide (NO2)

55
Q

which oxides containing nitrogen are colourless gases?

A

nitrogen monoxide (NO) and nitrous oxide (N2O)

56
Q

which gas containing nitrogen smells sweet?

A

nitrous oxide (N2O)

57
Q

if Ea increases k will….
this means the rate will….

A

get smaller
slow down

58
Q

when temperature increases k will…

A

increase

59
Q

what is seen when nitrogen monoxide gas reaches the atmosphere?

A

colourless gas turns brown

A Level Chemistry (12 decks)

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