The kinetics of a unimolecular reaction are observed and the reactant decays over time but it is not clear from the raw data whether the process is first-order or second-order. The two plots below represent fits to least-squares lines, with the equations shown. From this information, indicate the value of the rate constant. In [A]t -0.5H -net -1.5 -2.0 -2.5 -3.0 0 y = -0.00482 x - 1.11 R² = 0.894354 100 200 t (sec) 300 400 1 [A]t 20 15 10 5 0 y = 0.04039 x + 2.0267 100 200 R² = 0.999308 300 t (sec) 400

Calculate the instantaneous rate of the reaction (M/s), A + B ->C , where the rate constant is 5.64 x 102 M-1s-1? A has 0.054M concentration and the concentration of B is 0.043 M and the reaction is in second order relative to A and zero order relative to B. Balance the reaction as followsT TeO32- + N2O4 + H2O -> Te + NO3- + H+

[A] vs Time In[A] vs Time 1/[A] vs Time O Least Squares Plot Time, s The reaction A - C was performed and the concentration vs. time data below collected. time, s 2 3 4 5 7 8 [A], mol/L 0.9540 0.5864 0.3605 0.2216 0.1362 0.08371 0.05145 0.03163 0.01944 Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = k[A]* rate constant (without units) = reaction order = [v]uj

The rate of a reaction is monitored by measuring the number of moles of product that form per liter per second. The data obtained are listed in the table below. Using this data, mathematically determine the order with respect to each reactant, the overall order of the reaction, determine the rate constant, k, with units, and write the complete rate law. Experiment [X], M [Y], M Rate, Msec-1 1 0.0500 0.0850 0.643 2 0.0300 0.0850 0.386