Rates Flashcards

1
Q

Rate of reaction

A

How fast a reactant is being used up/product is being formed
Rate=change in conc/time
Fastest at start highest conc of reactant

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2
Q

Effective collision theory

A

2 reacting particles must collide with the correct orientation and sufficient energy in order for a reaction to occur

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3
Q

Catalyst

A

Substance that changes the rate of reaction without undergoing permanent change itself
Provides alternative pathways w lower activation energy

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4
Q

Enthalpy profiles

A

Endothermic reactants lower than products (enthalpy arrow up)
Exothermic reactants higher than products (enthalpy arrow down)

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5
Q

Homogenous catalyst

A

Same physical states as reactants
Forms an intermediate which breaks down to give the product and regenerates the catalyst
Eg sulphuric acid making an ester
Or Cl • radicals in ozone

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6
Q

Heterogenous catalysts

A

Different physical state from reactants
Reactant molecules are adsorbed onto surface
Products desorped
Eg Fe in haber process
No in hydrogenation of Alkene

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7
Q

Catalyst importance

A

Less fossil fuel is used making product faster w less energy increase profitability
High atom economies and fewer pollutants enzymes do this cutting co2 emissions due to less energy required

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8
Q

Boltzmann distribution curves

A

No molecules have zero energy curve starts at origin
Are under curve is equal to total number of molecules
Doesn’t touch x axis - no maximum energy

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9
Q

Temp x Boltzmann

A

At higher temp peak is lower and shifted to the right greater proportion can overcome activation energy

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10
Q

Catalyst x Boltzmann

A

Alternate route lowering the activation energy - greater proportion of molecules (closer to y axis)

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11
Q

Dynamic equilibrium

A

When the rate of the forward reaction is equal to the rate of the backwards reaction
Conc of products/reactants don’t change
Must occur in a closed system

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12
Q

Le Chatelier’s principle

A

When a system in equilibrium is subjected to an external change the system readjusts itself to minimise the effect of that change

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13
Q

Conc x equilibrium

A

If more products equlibrium shifts to the left
If more reactants equilibrium has shifted to the right

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14
Q

Temp x equilibrium

A

Increase in temp shifts equilibrium in endothermic direction
Decrease in temp shifts equilibrium in Exothermic direction

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15
Q

Equilibrium constant

A

Kc = products / reactants
(Number of moles = power of)

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