This questiоn is аbоut reаctiоn kinetics, integrаted rate laws, and temperature dependence. A reaction A -> products was studied by measuring [A] over time. The data are: time (min): 5, 10, 15 [A] (M): 0.38090, 0.23103, 0.14013 A separate first-order reaction B -> products has k = 9.60 x 10^-3 s^-1 at 45 degrees C. A second-order reaction C -> products has k = 1.80 x 10^-3 M^-1 s^-1 at 27 degrees C. Finally, for another reaction, increasing the temperature from 298 K to 310 K increases the rate constant by a factor of 2.50. A. Use the A data to decide whether the reaction is most consistent with zero, first, or second order. B. Calculate the first-order rate constant for A -> products using the data. C. For B -> products, calculate the time required for [B] to fall to 6.25 percent of its initial value. D. For the second-order reaction C -> products, calculate [C]0 if the half-life is 214 s. E. Estimate the activation energy for the reaction whose rate constant increases by a factor of 2.50 from 298 K to 310 K. F. Interpret why a reaction with a larger activation energy is more temperature-sensitive. G. Explain whether a catalyst would change the equilibrium constant for A -> products. Please do not enter anything in the text box below, but rather answer in writing on paper.
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