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
Reactor
Sulfur trioxide
3 (a) Complete and balance the equati... 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 formation of sulfur trioxide from sulfur dioxide and oxygen is:
2SO2(g)+O2(g)↔2SO3(g)
Step 2
State the effect of increasing the pressure on the rate of reaction.
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Answer
Increasing the pressure of the reacting gases increases the rate of the reaction.
Step 3
Explain your answer in terms of particles.
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Answer
When pressure is increased, the gas molecules are forced closer together. This results in a higher concentration of particles in a given volume, leading to an increased frequency of collisions between the reactant particles. More collisions increase the likelihood of successful reactions.
Step 4
Suggest and explain why shape B is more effective as a catalyst than shape A.
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Answer
Shape B provides a greater surface area compared to shape A. A larger surface area allows more gas molecules to simultaneously react with the catalyst, resulting in a faster reaction rate. The increased surface area facilitates more frequent interaction between the catalyst and the reactants.
Step 5
What is meant by the activation energy?
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The activation energy is the minimum amount of energy required for particles to collide and react effectively. It is the energy needed to break bonds in the reactants before new bonds can form to create the products.
Step 6
Explain why potassium would not be a suitable metal to react with sulfuric acid.
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Answer
Potassium is too reactive and can react violently with sulfuric acid. The reaction could produce hydrogen gas rapidly and create hazardous conditions, as well as potentially leading to violent explosions.
Step 7
Complete the equation for this reaction.
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Answer
The reaction can be completed as:
Zn+H2SO4→ZnSO4+H2
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.
