Question 1
Which statement correctly explains, using collision theory, why an increase in the concentration of reactants causes the rate of a chemical reaction to increase?
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Chemistry · Unit 2 · Rates of chemical reactions · Rates of reactions
Apply the collision theory to determine the effect of concentration, temper ature, pressure and surface area on the rate of chemical reactions.
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Question 2
A student prepares two samples of zinc powder and places them into separate beakers containing dilute hydrochloric acid at the same temperature. In Sample A, the zinc is finely powdered. In Sample B, the zinc is in the form of granules. Apply collision theory to explain why the reaction in Sample A is faster than the reaction in Sample B.
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Question 3
A reaction between zinc metal and dilute hydrochloric acid is performed at 25 °C. The rate of reaction is initially observed to be slow. Which change would increase the rate of reaction by increasing the frequency of effective collisions between reactant particles?
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Calculate the rate of chemical reactions by measuring the rate of formation of products or the depletion of reactants. (Formula: rate of reaction = increase in product concentration (∆[P]) time taken or decrease in reactant concentration (−∆[R]) time taken)