Question

Consider the following reactions:
$A \rightarrow P 1 ; B \rightarrow P 2 ; C \rightarrow P 3 ; D \rightarrow P 4$
The order of the above reactions are $a , b , c ,$ and $d$, respectively. The following graph is obtained when log [rate] vs. $\log [$ conc $]$ are plotted:

Among the following , the correct sequence for the order of the reactions is:

• A. a > b > c > d
• B. c > a > b > d
• C. d > b > a > c
• D. d > a > b > c

Answer 1

Answer: (C)

Rate law $R = K$ [conc.] $^{ n }[ n \rightarrow$ order $]$

$\log ($ Rate $)=\log K + n \log [$ conc.$]$

For log(rate) $v / s$ log [conc.] graph

[Slope $= n]$

As slope increases order (n) increases

$\therefore $ Order $d > b > a > C$