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44 Terms
1
reversible reaction
a reaction that can go both directions from reactants to products and products to reactants
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2
equilibrium
a state in a reaction where the rate of the forward reaction is equal to the rate of the backwards reaction
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3
forward reaction
reactants becoming products
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4
backwards reaction
the products reversing and becomin the reactants again
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5
what happens during a reversible reaction that makes the reaction into equilibrium
as the reactants react , their concentrations of the reactants fall so the rate of the forward reaction slows down
but as more and more products are made and their concentration rises, the rate of the backwards reaction will speed up
and so after a while the forward reaction and the backwards reaction will be going at exactly the same rate and so the system is in dynamic equilibrium
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6
dynamic equilibrium
a reversible reaction in a closed system where the forward and backwards reaction are occuring at the same rate
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7
closed system
a reaction where no reactants or products are able to escape or be introduced
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8
what does dynamic equilibrium mean for the concentrations of the reactants and products
the concentrations of the reactants will stay the same and the concentrations of the producst will stay the same
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9
what happens when the position of equilibrium lies to the right
means the concentration of products is greater than the reactants
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10
what happens when the position of equilibrium lies to the left
means the concentration of reactants is greater than the products
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11
what conditions does the position of the equilibrium depend on
temperature
pressure
concrentration of the reactants and the products
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12
endothermic
a reaction which takes in energy from the surroundings
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13
a reaction which gives out energy to the surroundings
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14
what are reversible reaction in relation to energy
one side will be endothermic and the other will be exothermic
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15
what is the energy on both sides to each other
the energy absorbed from the surrounding by the endothermic reaction is equal to the energy transferred to the surroundings by exothermic reaction
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16
Le Chatelier’s principle
a reversible reaction at equilibrium will try to counteract any change in conditions
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17
what happens to a reversible reaction at equilibrium when you increase the temperature
the equilibrium will shift to the endothermic side to try and decrease the temperature because endothermic takes in energy
this means that the concentration on the endothermic side will be greater
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18
what happens to a reversible reaction at equilibrium when you decrease the temperature
the equilibrium will shift to the exothermic side to try and increase the temp
this means the concentration on the exothermic side will be greater
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19
what state does cahnging the rpessure affect the equilibrium
only in gases
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20
what happens to a reversible reaction at equilibrium when you increase the pressure
the equilibrium will try to reduce the pressure so will shift to the side where there is less molecules of gas, where there is less moles
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21
what happens to a reversible reaction at equilibrium when you decrease the pressure
the equilibrum tries to increase it moves in the direction where there is more molecules of gas, where there is more moles
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22
moles is a measure of
how many molecules or atoms there are
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23
what happens if you change the concentration of either sides of the reaction
the system will no longer be at equilibrium so the system respnds by bringing it back to equilibrium
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24
what happens to a reversible reaction at equilibrium when you increase the concentration of the reactants
the system tries to decrease it by making more products
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25
what happens to a reversible reaction at equilibrium when you decrease the concentration of the products
the system tries to increase it by reducing the ampunt of reactants
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26
haber process
an important industrial process that produces ammonia from nitrogen and hydrogen
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27
why is the haber process well suited to industrial scale
nitrgoen is obtained easily- air is 78% of nitrogen
hydrogen mainly comes from reacting methan with steam
iron catalysts used, a high temp of 450 celsius and a high pressure of 200 atm
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28
what does the haber process reach because it is a reversible reaction
dynamic equilibrium
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29
stages of the haber process
Stage 1: H2and N2 gases are pumped into the compressor through pipes
Stage 2: The gases are compressed to about 200 atmospheres inside the compressor
Stage 3: The pressurised gases are pumped into a tank containing layers of catalytic iron beads at a temperature of 450°C. Some of the hydrogen and nitrogen react to form ammonia in the followingreversible reaction:
N2 (g) + 3H2 (g) ⇌ 2NH3 (g)
Stage 4: Unreacted H2and N2 and product ammonia pass into a cooling tank. The ammonia is liquefied and removed to pressurised storage vessels
Stage 5: The unreacted H2and N2 gases are recycled back into the system
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30
compromises made in the haber process
the forward reaction in haber process is exothermic so increasing the temp would make it go the wrong way, so the yield of ammonia would be greater at lower temp
lower temps mean slower rate of reaction
howerver increasing the pressure moves equilibrium over to the right so pressure is set as high as possibel without making it too expensive
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31
NPK fertilisers
formulations containing nitogen,phosphorous and potassium
helps to grow food
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32
why are formulated fertilisers better than using manure
more widely availbale
easier to use
dont smell
have just enough of each nutrient to grow
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33
how is ammonia used to make nitric acid
ammonia reacts with oxygen to make nitric acid and water
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34
ammonium salts
ammonia + acids
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35
what can ammonium salts be used as
fertilisers
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36
ammonium nitrate
ammonia + nitric acid
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37
ammonium nitrate production in industry
reaction carried out in giant vats, at high concentrations resulting in a very exothermic reaction
heat released is used to evaporate water from the mixture to make a very concentrated ammonium nitrate product
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38
ammonium nitrate production in the lab
much smaller scale by titration and crystallisation
reactants are at a much lower concentration than inindustry so less heat is produced and its safer
after titration, the mixture then needs to be crystallized to give the pure ammonium nitrate crystals
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39
how is potassium obtained
potassium chloride and potassium sulphate can be mined
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40
how is phosphate obtained
also mined however since the phosphat salts in the rock arent soluble, plants cant absorb phosphate
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41
how do you make phosphate rock soluble
react it with acid
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42
phosphate + nitric acid
phosphoric acid +calcium nitrate
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triple superphosphate
phosphoric acid+ calcium containg compound
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44
ammonium phosphate
ammonia+phosphoric acid
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