1)
see experiment 1 and 2:
[CH3NNCH3] becomes 2 times
rate becomes 2 times
so, order of CH3NNCH3 is 1
Rate law is:
rate = k*[CH3NNCH3]
2)
Put values from 1st row of table in rate law
rate = k*[CH3NNCH3]
2.8*10^-6 = k*0.0113
k = 2.48*10^-4 s-1
Answer: 2.48*10^-4 s-1
Example: CH3NNCH: (g) CH. (g) + N2 (8) In experiments on the decomposition of azomethine the following data wa Expe...
The decomposition of nitrous oxide at 565 °C N2O(g)----> N2(g) + ½ O2(g) is second order in N2O. In one experiment, when the initial concentration of N2O was 0.790 M, the concentration of N2O dropped to 0.103 M after 5.21×10^3 seconds had passed. Based on these data, the rate constant for the reaction is _____________ M-1 s-1.
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The following data were collected for the rate of disappearance ofNO in the reaction 2NO(g) + O2 --> 2NO2(g) : Experiment [NO] (M) [O2] (M) Initial Rate (M/s) 1 0.0126 0.0125 1.41 x 10-2 2 0.0252 0.0125 5.64 x 10-2 3 0.0252 0.0250 1.13 x 10 -1 (a) What is the rate law for the reaciton? (B) What are teh unitsof the rate constant? (c) What is the average value of the rateconstant calculated form teh three data sets? (d)...
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9,10,11
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