rates and equilibria Flashcards

1
Q

rate equation

A

rate = k [A]^m [B]^n
where [ ] is the equilibrium concentration and m/n is the order

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2
Q

order of 0

A

increase in concentration has no effect on rate of reaction

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3
Q

order of 1

A

increase in concentration and rate are directly proportional

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4
Q

order of 2

A

concentration and rate have a squared relationship

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5
Q

half-life

A

the time taken for the concentration of a reactant to decrease by half

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6
Q

k in terms of t1/2

A

k = ln 2 / t1/2

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7
Q

rate-determining step

A

slowest step of a reaction mechanism of a multi-step reaction

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8
Q

how to find the rate-determining step

A

the rate equation gives the species and their quantities in the rate-determining step

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9
Q

activation energy

A

minimum energy required to start a reaction by breaking bonds in the reactants

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10
Q

use of arrhenius equation on a graph

A

ln k = -Ea/R x 1/T + ln A
y-intercept gives ln A
gradient gives -Ea/R

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11
Q

le chatelier’s principle

A

when a system in dynamic equilibrium is subjected to a change in conditions, the position of equilibrium shifts to minimise the effect of the change

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12
Q

the equilibrium constant, Kc

A

Kc = [C]^c[D]^d / [A]^a[B]^b
where the lower case letters are the balancing numbers

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13
Q

homogenous equilibrium

A

all species are in the same state

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14
Q

heterogenous equilibrium

A

species are in different states

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15
Q

significance of Kc values

A

Kc < 1 equilibrium shifts left
Kc > 1 equilibrium shifts right

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16
Q

the equilibrium constant, Kp

A

Kp = p(C)^c x p(D)^d / p(A)^a x p(B)^b
where p is the partial pressure

17
Q

mole fraction

A

mole fraction of A = moles of A / total moles

18
Q

partial pressure

A

partial pressure = mole fraction x total pressure

19
Q

rate of reaction

A

change in concentration of reactant or product per unit time

20
Q

collision theory

A

molecules must collide with each other with energy greater than or equal to activation energy, with the correct orientation

21
Q

effect of increasing pressure on rate of reaction

A

gas molecules are pushed closer together
more gas molecules per unit volume
more frequent successful collisions
rate increases

22
Q

effect of increasing temperature on rate of reaction

A

kinetic energy of molecules increases
a higher proportion of molecules have energy greater than or equal to activation energy
more frequent successful collisions
rate increases

23
Q

types of catalysis

A

heterogenous catalysis - catalyst is in a different physical state than the reactants
homogenous catalysis - catalyst is in the same physical state as the reactants

24
Q

effect of a catalyst

A

increases the rate of reaction by providing an alternate reaction pathway with a lower activation energy

25
dynamic equilibrium
rate of forward and reverse reactions are equal system is closed concentration of reactants and products does not change
26
effect of pressure on position of equilibrium
if pressure is increased, the position of equilibrium will shift to the side with the fewest moles of gas (and vice versa)
27
effect of temperature on position of equilibrium
in de exothermic | L | R endothermic | R | L
28
effect of catalyst on position
catalyst increases the rate of the forward and reverse reaction equally so has no effect on the position of equilibrium