Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.93 M 0.265 M 0.319 M/s 1.93 M 0.0940 M 0.113 M/s 0.261M 0.265 M 0.00583 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0x15 ロ・ロ X

Consider the following data showing the initial rate of a reaction  (A → products) at several different concentrations of A.          [A] M        Initial Rate (M/s)  0.16               0.0141  0.32               0.0139  0.64               0.0140 What is the order of the reaction?     zero     first     second     third

Some measurements of the initial rate of a certain reaction are given in the table below. H2 2| initial rate of reaction 0.140M 1.66M 0.112 M/s 0.553 M 1.66M 0.442M/s 0.140M 0.418M 0.0282M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k ||| k = ?

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Some measurements of the initial rate of a certain reaction are given in the table below. N2 H2 initial rate of reaction 2.41M 2.25M 0.489M/s 6.14M| 2.25M 1.25M/s 2.41M 4.49M 1.95M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k|| x10 k =

Consider the following reaction data. Reaction [A] (M) [B] (M) Rate (M/s) 1 0.100 0.100 10 2 0.200 0.100 20 3 0.100 0.200 40 The generic rate law equation is: rate = k[A]x[B]y What is the value of y?

Determine the rate law and the value of k for the following reaction using the data provided.2 NO(g) + O2(g) → 2 NO2(g) [NO]i (M)      [O2]i (M)               Initial Rate (M-1s-1)0.030               0.0055                    8.55 × 10-30.030               0.0110                    1.71 × 10-20.060               0.0055                    3.42 × 10-2   Question options:   A)  Rate = 3.1 × 105 M-3s-1[NO]2[O2]2   B)  Rate = 9.4 × 103 M-2s-1[NO][O2]2   C)  Rate = 57 M-1s-1[NO][O2]   D)  Rate = 3.8 M-1/2s-1[NO][O2]1/2   E)  Rate = 1.7 × 103 M-2s-1[NO]2[O2]

Some measurements of the initial rate of a certain reaction are given in the table below. H2 12| initial rate of reaction 1.42 M 2.20 M 0.854 M/s 5.58 M 2.20 M 3.36 M/s |1.42 M 0.626 M 0.243 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol.

Some measurements of the initial rate of a certain reaction are given in the table below. [¹₂] H₂] initial rate of reaction 1.93 M 1.52M 66.0 M/s 0.476M 1.52M 4.01 M/s 1.93 M 0.412M Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k -0 17.9M/s k = X S

Some measurements of the initial rate of a certain reaction are given in the table below. H₂] [¹₂] initial rate of reaction 2.22M 2.20M 52.0 M/s 2.22M 0.389M 9.19 M/s 9.97M 2.20M 234. M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k x10 k = 0 00 Ś ?