n=1  rate = k [A]

Deducing a rate law from the change in concentration over time A chemistry graduate student is studying the rate of this reaction: 2C1,0, (g) → 2C1, (g) + 50, (g) He fills a reaction vessel with Ci,0, and measures its concentration as the reaction proceeds: time [C1,0,] (seconds) 0.0500M 10. 0.0170M 20. 0.0103 M 30. 0.00735 M 40. 0.00573 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k Calçulate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be ? sure your answer has the correct unit symbol.

Determine the rate law and the rate constant for this reaction. 13.125. The table contains reaction rate data for the reaction 2 NO(g) + Cl,(g)→ 2 NOCI(g) Initial Rate Experiment [NO], (M) [Cl_]o (M) (M/s) 1 0.20 0.10 0.63 0.20 О.30 5.70 0.80 0.10 2.58 0.40 0.20 Predict the initial rate of reaction in experiment 4. 13.126. An important reaction in the formation of photochemical smog is the reaction between ozone and NO: NO(g) + O3(g) → NO;(g) + O,(g) 2. 2. 3.

estimate the value of the rate constant k

Given the following rate and concentration data, determine the rate law for the reaction A + B ---> products [A]0 (M) [B]0 (M) initial rate (M/s) 0.10 0.10 4.22 X 10^-6 0.20 0.10 8.44 X 10^-6 0.20 0.40 3.38 X 10^-6 the rate constant k= rate=

Given the information below, determine the rate law for the reaction and the rate constant (k). Be sure to include the units for the rate constant (k). A + 2B --> C + D [A] M [B] M Initial Rate (M/s) 0.10 0.10 0.0015 0.20 0.10 0.0060 0.20 0.20 0.0120 0.40 0.10 0.0240 rate law: rate constant k:

Determine the rate law and the value of k for the following reaction using the data provided. 2 N205(g) 4 NO2(8) + O2(8) N205h (M) Initial Rate (M/s) 0.093 4.84 x 10-4 0.174 9.05 x 10-4 0.224 1.16 x 10-3 Rate = 6.0 x 10-1 M-25-1[N20513 Rate = 1.6 x 10-3 M1/25-1[N205]1/2 Rate = 5.2 x 10-3 s[N205] Rate = 1.7 x 10-2 M1/2s-1[N205]3/2 Rate = 5.6 x 10-2 M-151IN20512

Consider this reaction:                        A    +    B    →    C    +    D Expt. [A] (M) [B] (M) Initial Rate (M/s) 1 0.100 0.100 0.152 2 0.100 0.200 0.152 3 0.200 0.200 0.305   What is the overall reaction order for this reaction?

Determine the rate constant for the reaction 2 A + B - C [A] (M) [B] (M) Initial Rate (M/s) 0.05 0.05 0.035 0.10 0.05 0.070 0.20 0.10 0.56 O 2.8 x 102 M-2s-1 O 14 M-2s-1 O 1.4 x 102 M-2s-1 O 1.4 x 103 M-2s1