Figure 2 represents a reaction in the production of sulfuric acid - AQA - GCSE Chemistry - Question 3 - 2014 - Paper 1
Question 3
Figure 2 represents a reaction in the production of sulfuric acid.
Figure 2
Oxygen
Sulfur dioxide + Sulfur trioxide
Reactor
3 (a) Complete and balance the equa... show full transcript
Worked Solution & Example Answer:Figure 2 represents a reaction in the production of sulfuric acid - AQA - GCSE Chemistry - Question 3 - 2014 - Paper 1
Step 1
Complete and balance the equation for the reaction.
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Answer
The balanced equation for the reaction is:
ightarrow 2 SO_3(g)$$
Step 2
State the effect of increasing the pressure on the rate of reaction.
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Answer
Increasing the pressure increases the rate of reaction.
Step 3
Explain your answer in terms of particles.
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Answer
When the pressure is increased, the particles are forced closer together, leading to a higher frequency of collisions between them, which increases the rate of reaction.
Step 4
Suggest and explain why shape B is more effective as a catalyst than shape A.
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Answer
Shape B is more effective because it has a greater surface area compared to shape A. A larger surface area allows more reactant particles to collide with the catalyst at the same time, resulting in a faster reaction.
Step 5
What is meant by the activation energy?
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Activation energy is the minimum amount of energy that particles must possess in order to react or initiate a chemical reaction.
Step 6
Explain why potassium would not be a suitable metal to react with sulfuric acid.
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Potassium is a very reactive alkali metal that reacts violently with sulfuric acid, potentially leading to dangerous and uncontrollable reactions.
Step 7
Complete the equation for this reaction.
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Answer
The balanced equation for the reaction is:
ightarrow ZnSO_4 + H_2$$
Step 8
State one way, other than using a catalyst, that the student could increase the rate of the reaction.
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Answer
One way to increase the rate of reaction is to increase the concentration of sulfuric acid.
