rate law

Some measurements of the initial rate of a certain reaction are given in the table below. [N-] H2 initial rate of reaction 0.539M 0.871M 7.00 x 10°M/s 0.539M 0.282M 7.34 x 10*M/s olo 0.172M 0.871M 7.13 x 10*M/s Ar 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 =

A reaction between substances A and B has been found to give the following data: 3A +2B 2C+D Al (mol/L) (mol/Rate of appearance of C 10 x 102 10 x 102 30 2.0 x 102 30 mol / L-hr) 0.300 x 100 810x 10 3 24 x 10-5 1.20 x 10-8 30 x 10-5 10 0 x 102 1.0 3.0 x 10- Using the above data, determine: a) the order of the reaction with respect to A and B - b) the rate law, and - c) calculate the specific rate constant

Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. [H₂] [2] initial rate of reaction 1.96M 1.54M 0.939 M 1.54M 1.96M 0.618M 4.00 × 104 M/s 1.92 × 10 M/s 1.61 × 104 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 = 0 □·□ 吕

The kinetic data shown below were observed for the reaction:    BF3 (g)     +   NH3 (g)    --------->      F3B·NH3 (g)   Trial # [BF3] (mol/L) [NH3] (mol/L) Rate (M/s) 1 0.250 0.250 0.2130 2 0.250 0.125 0.1065 3 0.200 0.100 0.0682 4 0.350 0.100 0.1193 5 0.175 0.100 0.0596 What is the rate constant for this experiment?

A chemistry graduate student is studying the rate of this reaction: 2C1,0, (3) – 2Cl, (g) +50, (g) She fills a reaction vessel with Cl,0, and measures its concentration as the reaction proceeds: time [CLO,] (seconds) 1.00 M 10. 0.666 M 20. 0.443 M 30. 0.295 M 40. 0.196 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k O Calculate 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 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

Write the rate law for the reaction of carbon monoxide and chlorine to form phosgene using the following data. CO(g) + Cl2(g) ⟶COCl2(g) Trial [CO]i [Cl2]i Rate (M/s) 1 1.00 0.100 1.29x10-29 2 0.100 0.100 1.33x10-30 3 0.100 1.00 1.30x10-29 4 0.100 0.0100 1.32x10-31 Group of answer choices rate = 4.21x10-29 s-1[Cl2] rate = 3.94x10-29 s-1[CO] rate = 6.84x10-30 M-1⋅s-1[CO][Cl2] rate = 6.84x10-30 s-1[CO] rate = 6.84x10-30 s-1[Cl2] rate = 1.31x10-28 M-1⋅s-1[CO][Cl2]

A scientist evaluated reaction rates for the reaction A + B --> C using differing initial concentrations of A and B and collected the following data: [A] [B] Rate 0.492 0.430 2.339 0.492 0.860 4.678 0.984 0.430 9.356 0.984 0.860 18.712 a) What is the rate order for reactant B in the rate law for this reaction?

For the chemical reaction NO2(g) + CO(g) → NO(g) + CO2(g) The following initial rate data were obtained Initial [NO₂] Initial [CO] Initial Rate Experiment (mol/L) (mol/L) (mol/L.s) 1 0.10 0.10 0.0050 2 0.40 0.10 0.080 3 0.10 0.20 0.0050 What is the rate law for the reaction? R = k [NO₂]4[CO] R = k [NO₂][CO] R = k [NO₂]²[CO] none of the answers are correct OR = K [NO₂]²