Consider the following reactions A → P1; B → P2; C → P3; D → P4 The...

Consider the following reactions
$A \to P1; B \to P2; C \to P3; D \to P4$
The order of the above reactions are $a, b, candd,$ respectively. The following graph is obtained when log[rate] vs.log[conc.] are plotted:

Consider the following reactions A → P1; B → P2; C → P3; D → P4 The order of the above reactions are a, b, candd,
Among the following, the correct sequence for the order of the reactions is :

Options

A $d > a > b > c$
B $a > b > c > d$
C $c > a > b > d$
D $d > b > a > c$

Correct answer

D. $d > b > a > c$

Step-by-step solution

Rate $= K [ Conc{]}^{\text{order}}$

logRate $= logK +$ $order \times log [ conc ]$
so slope of graph is order of reaction. greater the slope greater is order of reaction so order of reaction $⇒ " c < a < b < {d}^{' '}$

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