The rate of reaction between butanone and iodine is studied. In this experiment, butanone is in excess. The concentration of iodine is measured every 10 minutes for 1 hour. The results are shown in the table.

a. Plot these data on a suitable graph.

b. Show from the graph that these data are consistent with the reaction being zero order with respect to iodine.

c. The balanced chemical equation for the reaction is CH₃CH₂COCH₃ + I₂ → CH₃CH₂COCH₂I + HI

Could this reaction occur in a single step? Explain your answer.

d. The rate equation for the reaction is rate = k[CH₃CH₂COCH₃]

Explain the different meanings of the balanced chemical equation and the rate equation.

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Time / min 10 20 30 40 50 60 [L]/moldm3 0.060 0.051 0.041 0.032 0.022 0.012 0.003