the reaction: 4 Hrvo,le) 2NOdg) 2NO (a) 2H-O(e) (ql (Rate law HNO P). The chemic

Question

the reaction: 4 Hrvo,le) 2NOdg) 2NO (a) 2H-O(e) (ql (Rate law HNO P). The chemicaf kinetics data based concentration of HNO, at 520 K are given as follows on the instantaneous Time (hour) [HNO) M (mot/) 0.0000 5.000 1.270 1.008 0.800 0.635 0.504 10.000 In [HNO, 15.000 20.000 25.000 (a) (3pt) From the two plots in Figure 2, determine the reaction order x of reactant HNO? (b) (4pt) Cakculate the corresponding rate constant, for this reaction. íc) (3pt) Determine the haif life of the decomposition reaction of HNO, with the initial concentration HNO ]-1.600 M. time (hrs) 1.4 10 15 20 25 time (hrs) Figure 2

Explanation / Answer

a. the order of the reaction is first order because it maintains the first order reaction kinetics law. and by calculating the rate constant with consequtive points giving same value. That confirms the first order kinetics.

b. From the first order rate equation, K=2.303/t * log[a/(a-x)]

by taking first two data,

K=2.303/5 * log [1.600/(1.600-1.270)] = 2.303/5 * log [1.600/0.330] = 2.303/5 * 0.686 = 0.315 h-1

you can take any two consecutive differences you will get the same rate constant.

c. Now we know that Half-life(t1/2) = 0.693/K = 0.693/0.315= 2.2 h

so

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