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6 (a) A student investigated the rate of a reaction - Edexcel - GCSE Chemistry - Question 6 - 2013 - Paper 1
Question 6
6 (a) A student investigated the rate of a reaction. The student investigated the reaction between zinc and dilute sulfuric acid. The products are zinc sulfate, ZnSO... show full transcript
Worked Solution & Example Answer:6 (a) A student investigated the rate of a reaction - Edexcel - GCSE Chemistry - Question 6 - 2013 - Paper 1
Step 1
Step 2
Evaluate these results, explaining the reasons why the rate of reaction in experiment 2 is faster than the rate of reaction in experiment 1.
Answer
In experiment 1, the concentration of sulfuric acid is lower (0.5 mol dm⁻³) compared to experiment 2 (1.5 mol dm⁻³). A higher concentration means there are more acid particles present, which increases the likelihood of collisions with zinc particles.
Additionally, the temperature in experiment 2 is higher (40 °C) than in experiment 1 (20 °C). Raising the temperature increases the energy of the particles, resulting in more effective collisions. Thus, the rate of reaction in experiment 2 is faster due to both increased collision frequency and higher energy of the particles, leading to more successful reactions.
Step 3
Step 4
This reaction is exothermic. On the diagram below draw labelled lines to show the relative energies of the reactants and products in this reaction.
Answer
In an exothermic reaction, the energy of the products is lower than the energy of the reactants. Therefore, on the diagram, draw a line starting at a higher point representing the reactants and ending at a lower point for the products, indicating the release of energy during the reaction.