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chemical industry Flashcards

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1
Q

what does the rate of reaction measure

A

the rate of reactant→product conversion

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2
Q

formula for rate

A

rate = amount of reactant used or product made / time

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3
Q

use of rate equation

A

can be used to calculate the rate of reaction from concentrations and a known constant for a given temperature

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4
Q

rate equation

A

rate = k[A]^a [B]^b
[A] [B] = concentration of reactants
a b = orders of reactant

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5
Q

orders of reaction meaning

A

the power to which a concentration is raised to in the rate equation

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6
Q

zero order meaning

A

changes in concentration has no effect on rate

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7
Q

first order meaning

A

changes in concentration has a proportional change on the rate
e.g. if [A] doubles, rate doubles

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8
Q

second order meaning

A

changes in concentration has a squared proportional change on the rate
e.g. if [A] doubles, rate quadruples

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9
Q

features of rate constant - k

A
  • only fixed at a particular temperature
  • larger value of K, the faster the reaction
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10
Q

finding rate on a concentration time graph

A

rate is found by taking the gradient

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11
Q

zero order on a concentration time graph

A

\
diagonal line from top to bottom

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12
Q

zero order on a rate concentration graph

A

_
horizontal line, as changing concentration doesn’t affect rate

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13
Q

first order on a concentration time graph

A

slight curved slope doing down as time increases, eventually plateaus (not very steep)

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14
Q

first order on a rate concentration graph

A

/
straight diagonal line going up, as changing concentration changes rate equally

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15
Q

second order on a concentration time graph

A

curved slope doing down as time increases, eventually plateaus (steep)

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16
Q

second order on a rate concentration graph

A

curved line going up
changing concentration changes the rate squared

17
Q

half life definition

A

the time it takes for half of the reactant to be used up

18
Q

half life of zero order

A

half life decreases

19
Q

half life of first order

A

half life is constant

20
Q

half life of second order

A

half if increases

21
Q

formula to calculate half life from rate constant

A

k = ln2 / half life

22
Q

arrhenius equation for graphs

A

lnK = (-Ea/R) 1/T + lnA

23
Q

arrhenius equation meaning

A

k = rate constant
A = arrhenius constant
e = exponential (on calculator)
Ea = activation energy
R = gas constant
T = temperature (in K)

24
Q

what is the rate determining step

A

the slowest step in a multi-step reaction
the whole reaction rate depends on how quick the rds is

25
Q

features of the rate equation

A
  • reactants that appear in the rate equation affect the rate reaction
  • these reactants (or substances derived from them) must appear in the rate determining step
26
Q

what are reversible reactions

A

reactions that can go forward and backward

27
Q

features of a reversible reaction

A
  • dynamic equilibrium reached when rate of forward = rate of backward
  • concentration of substance remains constant
  • only occurs in closed systems
28
Q

what affects value of Kc

A

only temperature

29
Q

temperature affect on Kc

A
  • changing the temperature will change equilibrium concentrations
  • if temperature change causes equilibrium to shift to right, Kc will increase
  • if temperature change causes equilibrium to shift left, Kc will decrease
30
Q

Kc expression

A

[products] / [reactants]

31
Q

what is Kc

A

the equilibrium constant

32
Q

Kc expression of
2A + B <==> 2C + D

A

Kc = [C]^2 [D] / [A]^2 [B]

33
Q

features of nitrogen

A
  • diatomic molecule
  • in group 5
  • 1s2 2s2 2p3
  • forms a covalent triple bond (very difficult to break and so nitrogen is an unreactive gas at room temperature)
34
Q

common nitrogen molecules

A
  • ammonia (NH3)
  • ammonium (NH4+)
  • nitrogen monoxide (NO)
  • dinitrogen oxide (N2O)
  • nitrogen dioxide (NO2)
35
Q

features of ammonia

A
  • NH3
  • formed by N2 + H2
  • formed in Haber process
  • Nitrogen shares 3 of its valence electrons with hydrogen and a lone pair of electrons remain
  • due to lone pair, ammonia can form hydrogen bonds with water so it is very stable
  • ammonia can form dative covalent bonds using lone pair, e.g. to form ammonium ion
36
Q

raw materials meaning

A

chemical companies will try and source raw materials that are cheap and widely available

chemistry (8 decks)

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