Question

10. Some measurements of the below. a certain reaction are given in the table 0.413 M 2.41 M 0.750 M 2.41 M 0.413 M 0.960 M initial rate of reaction 5 .00 x 10mis 1.65 x 10° Mls L 7.93 104 m/s 77 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=

Answer 1

+ N2 experiment H2 initial N2 0.413 [ ] [ initial H2 ] 2.410 2.410 0.960 initial rate initial rate | M/S M/S 5.00x105 500000.0 1.65x106 1650000.0 7.93x104 79300.0 0.750 0.413 | order with respect to N2 order with respect to H2 rate of reaction = k [ N2 = x = y ][ H2 ] to determine the order with respect to N2 ( experiment 2 ) 1650000.0 = { [0.750 ] [ 2.410 ]Y ( experiment 1 ) 500000.0 = { [0.413 ] [ 2.410 ]Y 1650000.0 1 0.750 X 500000.0 0.413) 3.30 = 1 1.82 ) x = 2 I experiment 3 ) 79300.0 = k [0.413 ] [ 0.960 ] ( experiment 1 ) 500000.0 = k [0.413 ] [ 2.410 ] 79300.0 10.960 y 500000.0 2.410 0.16 = ( 0.40 )* y = 2

order with respect to N2 = 2 order with respect to H2 = 2 overall order of the reaction = 4 rate of reaction = k[ N2 l?[ H2] rate of reaction = k [ N2 ] [ H2 1² 500000.0 = k [ 0.413]2[ 2.410 ] k = 504702.9 M-3.5-1 k = 5.05x105 M-3.5-1