3-6. Lee (1990) reported the following data for the oxi- dation of acetic acid by hydrogen peroxide under supercritical conditions (T> 374C, P>218 bar) in a batch system. The first table contains data collected at T close to 500C, and the second table contains data over a range of temperatures. Experimental results for variable reaction times at (approximately) the same temperature Temperature (C) 40 (mmol/L) 1 (mmol/L) Time (s) 502.7 501.0 5023 503.7 2.925 2.822 2.815 2.804 0.313 0.468 0.152 0.056 13.7 14.1 20.2 26.0 Experimental results for systems at different temperatures Temperature (C) 40 (mmol/L) 1 (mmol/L) Time (s) 450.9 3.877 1.935 29.3 449.0 5.369 3.425 20.7 461.7 3.509 1.323 27.6 462.7 3.239 1.189 26.0 473.9 3.250 0.546 32.1 474.9 3.242 0.486 32.2 5023 2.815 0.152 20.2 503.7 2.804 0.056 26.0 523.9 1.555 0.023 14.1 525.5 1.528 0.015 20.6 (a) Use integral methods to determine whether the data are best described by zero, first, or second- order reaction kinetics with respect to acetic acid, and estimate the rate constant for the chosen rate expression. (Note: these data are messy. Consider the implicit data point at time zero in addition to the reported data to aid in the analysis.) (b) Based on the reaction order determined in parta, estimate the value of the rate constant k for each experiment in the second table, and estimate the value of Ear for the reaction