Give the data below, and for the reaction X + Y→ Z, which of the following is consistent with the rate law? Experiment # 1 2 3 4 5 [X] (M) 0.1 0.1 0.5 0.3 0.5 [Y] (M) 0.4 0.2 0.4 0.4 0.4 The reaction is a bimolecular collision of 2 X molecules. The reaction is a unimolecular event involving 1 X molecule. The reaction is a bimolecular collision of 2 Y molecules. [Z] (M) 0.1 0.1 0.1 0.2 0.2 The reaction is a bimolecular collision of 1 Y molecule and 1 X molecule. Rate 1.2 x 10-3 3.0 x 10-4 1.2 x 10-3 1.2 x 10-3 1.2 x 10-3

For the following reaction 2A > A2 This is a zero rate order. The rate constant is y = -0.0034x +0.9996 What is the rate law expression? What is the concentration at 290 seconds? Time [A](M ) 0 1 25 0.914 50 0.829 75 0.744

From the data given in the table below, determine the rate law for the following chemical equation. NH4+(aq)  +  NO2-(aq)  →  N2(g)  +  2 H2O(l)     Experiment        [NH4+]o                [NO2-]o                 Initial Rate (consumption of NH4+) 1                           0.24                     0.10                         7.2 x 10-6 M/s 2                           0.12                     0.10                         3.6 x 10-6 M/s 3                           0.12                     0.15                         5.4 x 10-6 M/s   Select one: a. Rate = k[NH4+][NO2-]2 b. Rate = k[NH4+]2[NO2-] c. Rate = k[NH4+]2 d. Rate =k[NH4+]2[NO2-]2  e. Rate = k[NO2-] f. Rate = k[NO2-]2 g. Rate = k[NH4+] h. Rate = k[NH4+][NO2-]

The reaction A -C was performed and the concentration vs. time data below collected. time, s 1 2 3 4 5 6 7 [A], mol/L 0.9088 0.5902 0.3833 0.2489 0.1617 0.1050 0.06818 0.04428 0.02876 Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = k[A]X rate constant (without units) = reaction order =