The reaction A (aq) → products was studied at 25∘C. Initial rate data were collected for five trials in which only the initial concentration of A was varied.
Trial | [A]0 (M) | Initial rate (M s−1)
1 | 0.050 | 3.2×10−6
2 | 0.075 | 5.6×10−6
3 | 0.100 | 8.5×10−6
4 | 0.150 | 1.7×10−5
5 | 0.200 | 2.4×10−5
(1) Part 1: (a) For each trial, calculate log([A]0) and log(rate). Record the values to three significant figures.
(2) Part 2: (b) Using any two appropriate trials, determine the numerical value of the exponent that relates the initial concentration of A to the rate.
(3) Part 3: (c) Use your result from part (b) to determine the order of the reaction with respect to A and write the corresponding rate law, leaving the rate constant expressed as k.
(4) Part 4: (d) Based on the order obtained in part (c), state the units that the rate constant k must possess.