Question

Consider the following data to answer the next 4 questions.

[A] initial (M) [B] initial (M) Initial speed of the reaction (M / s)

0.2 0.1 5

0.2 0.2   20

0.6 0.4 80

4a. The order of the reaction with respect to [A] is__________.

4b. The order of the reaction with respect to [B] is__________.

4c. The net order of the reaction s__________.

4d. The value of k is (include units) is__________.

Answer 1

data S.NO. CA initial M speed m/s (BJinitial 0.1 0.2 0.2 0.2 3 0.6 0.4 80 sate = k [A]ª[B]* where = {ate constant a= Order of rxn workit A and b= order of {Xn W. &.t. B. Overall order = arb we can see that on doubling the concentration of B lie. [B] the rate is increased 4 times, this means that order of reaction is a w.rit. [8] as (2) * = 4 and if we increase the concentration of A 3 times and cons of B to y times then rate changed or increased 16 times (i.e. from 5 to 80). effect of (B) = (2)" = 16, thus the all increased sate 15 due to B only and hence concentration of A don't have any effect on rate of reaction de order is zero w.rit. A. 4 (a) Order of reaction w.got. [A] = 0 u (6). Order of reaction w.a.t. [B] = 2 Overall order of reaction = ord = 2 40) R= rate 5 Mi 5 M/S = = 500 m's [A]°(B) 2 (0.2)°(0.10 & Txo.olm²- kindly sute the answer !!! thank you. u (C).