Rates Flashcards

1
Q

what are units for rates?

A

moldm-3s-1

change in conc/time

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2
Q

at what time is the initial rate

A

0s
this is directly related to the initial concentration of the reactant

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3
Q

the rate equation for a general reaction
A + B -> C + D

A

rate = k [A]m[B]n

m = order of reaction with respect to reactant A
n = order of reaction with respect to reactant B

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4
Q

what is the order of reaction

A

m + n
the power to which the concentrations of this reactant is raised in a rate equation

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5
Q

zero order

A

the conc of a zero order reactant has no effect on the rate of reaction
[A]0 = 1

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6
Q

how to work out the rate of a reaction

A

it can only be found experimentally

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7
Q

first order

A

rate is proportional to A
so doubling A, doubles the rate of reaction

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8
Q

second order

A

rate is proportional to [A]2
if we double [A], the rate is quadrupled

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9
Q

what is the order of reaction

A

the power which [A] is raised with respect to A

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10
Q

what is the rate determining step

A

the slowest step that holds everything else up

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11
Q

measuring rates of reaction experimentally
Collecting gas

A

1) gas syringe is attached to a sealed reaction vessel and measure the volume of gas produced
2) measured on a graph against time
3) gradient of tangent shows the rate of reaction

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12
Q

measuring rate of reaction experimentally:
measure colour change using a colorimeter

A
  • if a blue solution you should use a red filter, as the solution is absorbing red light
  • amount of red absorbed relates directly to the concentration
  • draw a calibration curve, so absorbance can be converted to conc
  • several experiment take place with differ conc
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13
Q

measuring rate of reaction experimentally:
quenching and titrating

A
  1. The reaction in each of the samples is stopped (quenching)
  2. Quenching ‘freezes’ the reaction to allow the concentration to be determined by titration
  3. with collected data, the ror can be calculated by determining the change in concentration with time
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14
Q

measuring rate of reaction experimentally
loss of mass

A
  • measuring mass over a period of time. curve decrease until initial tangent T=0s gives the initial rate
  • conc will be changed and initial rate is measured
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15
Q

measuring rate of reaction experimentally
ph monitoring

A

pH = -log10[H]+, so [H]+ = 10(-pH)
- pH values can be taken over time, they can be directly converted to [H]+ by using the equation
-graph of [H]+ can be drawn
- if [H]+ is a reactant, the curve can give the rate or gradients of tangents at various [H]+ can be taken which equal the rate

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16
Q

the Arrhenius equation

A

links the rate constant with activation energy and temperature
K= Ae -Ea/RT

K = rate constant
A = frequency factor
e = mathematical quantity
Ea = activation energy (Jmol-1)
R = gas constant
T = temperature (Kelvins)

17
Q

relationship between K and the rate

A

whatever k increase by the rate increase by the same factor
e.g. double

18
Q

Arrhenius equation
finding the activation energy (Ea)

A

Ea = (InA x RT) - InK

19
Q

Arrhenius equation
finding the frequency factor (A)

A

A = K/e -Ea/RT

20
Q

Arrhenius equation
finding the temperature (T)

A

InA - Ea / Ink x R

21
Q

Arrhenius equation
finding InK

A

InK = InA - Ea/RT