Aspirin,C9H8O4, slowly decomposes at room temperature by reacting with water in

Question

Aspirin,C9H8O4, slowly decomposes at room temperature by reacting with water in the atmosphere to produce acetic acid, C2H4O2, and 2-hydroxybenzoic acid, C7H6O3 (this is why old bottles of aspirin often smell like vinegar): C9H8O4(s) +H2O(g) -> C2H4O2(l) +C7H6O3

By using the Collision Model of Chemical Kinetics and an atomic-scale view, describe what effect(s) an incrase in each of the following is expected to have on the rate of the reaction.

a. temperature

b. concentration of water vapor

c. activation energy

and thank you

Explanation / Answer

C9H8O4(s) +H2O(g) -> C2H4O2(l) +C7H6O3

a. According to collision model, as the temperature increases the collision between reactant molecules also increases which helps to cross the energy barrier easily to form products. Thus the rate of reaction increases as the temperature increase.

b. As the concentration of water vapour increases the probability of collision with other reactant increase which leads to increase the rate of reaction.

c. As the activation energy increase the reactants can easily cross the energy barier and leads to increase the rate of reaction.

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