Kinetics 5 Flashcards

1
Q

collision theory

A

for a reaction to take place between two particles, they must collide with enough energy to break bonds

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2
Q

factors that affect the rate of a chemical reaction

increasing the temperature

A

increases the speed of the molecules which in turn increases the energy and number of collisions

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3
Q

factors that affect the rate of a chemical reaction

increasing the concentration of a solution

A

more particles are present in a given volume then collisions are more likely and the reaction rate would be faster. however, as a reaction proceeds, the reactants are used up and their concentration falls. so, in most reactions, the rate of reaction drops as the collisions are more likely

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4
Q

factors that affect the rate of a chemical reaction

increasing the pressure of a gas reaction

A

there are more molecules or atoms in a given volume so collisions are more likely

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5
Q

factors that affect the rate of a chemical reaction

increasing the surface area of solid reactants

A

greater the total surface area, more of the particles are available to collide with molecules in a gas or liquid

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6
Q

factors that affect the rate of a chemical reaction

using a catalyst

A

a catalyst is a substance that can change the rate of chemical reaction without being chemically changed itself

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7
Q

maxwell-Boltzmann distribution

A
  • no particles has zero energy
  • most particles have intermediate energies
  • a few have very high energies
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8
Q

activation energy

A

reaction to take place, a collision between particles must have enough energy to start breaking bonds.
the area under the line represents the number of particles with enough energy to react.

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9
Q

effect of temperature on the rate of reaction

A

at high temperature, the peak of the curve is lower and moves to the right. the number of particles with very high energy increases.

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10
Q

catalysts

A

provide a different pathway for the reaction, one with a lower activation energy

Don’t get used up in the reaction

(A catalyst is a substance that increases the rate of a chemical reaction without being changed in chemical composition or amount)

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11
Q

what catalyst does the Haber process use ( and uses)

A
  • iron

- making fertilisers

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12
Q

catalyst and uses of

4NH3 + 5O2 — 4NO +6H20 (nitric acid)

A
  • platinum and nickel

- making fertilisers and explosives

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13
Q

catalyst and uses of

hydrogenation

A
  • nickel

- margarine

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14
Q

catalyst and uses of cracking hydrocarbon chains from crude oil

A
  • aluminium oxide and silicon dioxide zeolite

- making petrol

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15
Q

catalyst and uses of the catalytic converter reactions in car exhausts

A
  • platinum and rhodium

- removing polluting gases

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16
Q

catalyst and uses of hydration of ethene to produce ethanol

A
  • H+ absorbed on solid silica, phosphoric acid (H3PO3)

- making ethanol;

17
Q

catalyst and uses of esterification

A
  • H+

- Making solvents

18
Q

catalytic converter

A
  • reduce levels of a number of polluting gases.
  • honeycomb made of ceramic material coated with platinum and rhodium metals

carbon monoxide + nitrogen oxides — nitrogen + carbon doixide

hydrocarbon + nitrogen oxide — nitrogen + carbon dioxde + water

19
Q

Zeolites

A

Mineral
Open pore structure
48 are naturally formed
Used in petrochemical industry

20
Q

Hardening

A

Unsaturated fat (margarines)
Hydrogen added
Nickel catalyst
Nickel filtered off at the end

21
Q

Catalyst and ozone layers

A

CFC were used (in sovalent / aerosol propellants)
Unreactive until UV

(Nitrogen monoxide acts a catalyst)

22
Q

Rate of reaction

A

Amount of reactants used / time

Reaction rate, the speed at which a chemical reaction proceeds

23
Q

Dynamic reaction

A

Closed system

Constant temperture

24
Q

Le chateliers principle

A

If a reaction at equilibrium is subjected to a change in concentration,pressure or temperature, the position of equilibrium will move to counteract the change

25
Q

N2O4 ↔️ 2NO2. +57.2kjmol-1

A

NO2 brown
N2O4 colourless

If you change the pressure then the colour changes because it would prefer on side

26
Q

Ethanol

C2H4 + H2O ↔️ C2H5OH

-46Kjmol-1

A

60-70 atmospheres
300 degrees
Phosphoric acid catalyst

To save money / materials - un reactive ethene is separated and recycled back into the reactor

27
Q

Methanol

2H2 + CO ↔️ CH3OH

A

50-100 atmospheres
250 degrees
Copper / zinc oxide / aluminium oxide

28
Q

Change in concentration

A

More reactant = more product

More product = more reactants

29
Q

Change in pressure

A

Only affects gases

Increase in pressure = favours the side with less moles

30
Q

Change in temperture

A
Increase temperature (add heat)
Shifts in the endothermic direction to a absorb the heat
Decrease temperature (remove heat)
Shifts to the exothermic to replace the heat
31
Q

why do most collisions do not lead to a reaction ?

A

do not have appropriate orientation to one another in the collision to lead to a reaction. Reactants must have enough energy to overcome the activation energy barrier in order to become products.