-Using the data in the table, calculate the rate constant of this reaction. A+B C+D k = Trial [A] (M) [B] (M) Rate (M/s) 1 0.230 0.370 0.0147 2 0.230 1.04 0.115 3 0.391 0.370 0.0250 Units

Using the information in the table, the value of the rate constant for the reaction A(g) + 3 B(g) → C(g) + 2 D(g) is

The data below were collected for this reaction: CH3Cl (g)         +     3 Cl2(g)     →        CCl4 (g)              +              3 HCl (g)   Expt. [CH3Cl] (M) [Cl2] (M) Initial Rate (M/s) 1 0.050 0.050 0.014 2 0.100 0.050 0.029 3 0.100 0.100 0.057   Provide the rate law for this reaction. Include the numerical value of the specific rate constant, k.     Rate = - Δ [Cl2]3 / Δ t     Rate = Δ [HCl] / 3 Δ t     Rate = k [CH3Cl] [Cl2]2     Rate = -Δ [CH3Cl] / 3 Δ t     Rate = 5.7 [CH3Cl] [Cl2]

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-]