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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 the first experiment, the concentration of sulfuric acid is 0.5 mol dm⁻³, while in the second experiment it is 1.5 mol dm⁻³. Higher concentration of reactants generally leads to more frequent collisions between reactant particles.
Additionally, the temperature in the second experiment is 40 °C compared to 20 °C in the first. Increasing the temperature increases the kinetic energy of the particles, resulting in more energetic and frequent collisions.
Thus, the combination of a higher concentration of sulfuric acid and a higher temperature in the second experiment leads to an increased frequency of collisions and greater energy during these collisions, resulting in a higher rate of reaction.
Step 3
Step 4
On the diagram below draw labelled lines to show the relative energies of the reactants and products in this reaction.
Answer
In this exothermic reaction, the energy of the products is lower than that of the reactants. Draw a labelled line starting from a higher point (representing reactant energy) to a lower point (representing product energy) and indicate 'heat energy released' in this drop.