Reversible Reactions

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What is a closed system?
Where no products or reactants can escape
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For a reversible reaction in a closed system, when is equilibrium reached?
When the rate of the forward reaction is equal to the rate of the reverse reaction and the amount of reactants and products remain constant
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What happens when you increase the concentration of a reactant?
It will cause more products to be formed as the system tries to achieve equilibrium
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What happens if a product is removed?
More reactants will react to try and achieve equilibrium so more product is formed
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What happens if we change the conditions of a system at equilibrium?
The position of equilibrium shifts as if to try cancel out the change
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If the forward reaction produces more molecules of gas, what happens if there is an increase of pressure?
There is a decrease in the amount of products formed
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If the forward reaction produces more molecules of gas, what happens if there is an decrease of pressure?
There is an increase in the amount of products formed
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If the forward reaction produces fewer molecules of gas, what happens if there is an increase of pressure?
There is an increase in the amount of products formed
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If the forward reaction produces fewer molecules of gas, what happens if there is an decrease of pressure?
There is a decrease in the amount of products formed
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If the forward reaction is exothermic what happens if the temperature increases?
There is a decrease in the amount of products formed
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If the forward reaction is exothermic what happens if the temperature decreases?
There is an increase in the amount of products formed
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If the forward reaction is endothermic what happens if the temperature increases?
There is an increase in the amount of products formed
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If the forward reaction is endothermic what happens if the temperature decreases?
There is a decrease in the amount of products formed
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What is the Haber process used to manufacture?
Ammonia which can be used to make fertilisers
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What are the conditions for the production of ammonia?
450C, pressure of 200 atmospheres and an iron catalyst
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What is the yield of ammonia?
15%
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What is the optimum pressure for the Haber process?
The products have fewer molecules of gas than the reactants, so the higher the pressure is, the greater the yield of ammonia
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Why are very high pressures not used for the Haber process?
Because the higher the pressure is, the ore energy is needed to compress the gas and they need stronger reaction vessels and pipes which increase costs
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What is the optimum temperature for the Haber process?
The forward reaction is exothermic, so the lower the temperature, the greater the yield of ammonia
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Why are low temperatures not used for the Haber process?
The rate of reaction decreases as the temperature is lowered and the iron catalyst becomes ineffective so it would take a longer time to produce any ammonia
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Other cards in this set

Card 2

Front

For a reversible reaction in a closed system, when is equilibrium reached?

Back

When the rate of the forward reaction is equal to the rate of the reverse reaction and the amount of reactants and products remain constant

Card 3

Front

What happens when you increase the concentration of a reactant?

Back

Preview of the front of card 3

Card 4

Front

What happens if a product is removed?

Back

Preview of the front of card 4

Card 5

Front

What happens if we change the conditions of a system at equilibrium?

Back

Preview of the front of card 5
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