Consider the following reactions $A \to P 1; B \to P 2; C \to P 3; D \to P 4$ , 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

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$d > a > b > c$

$a > b > c > d$

$d>b>a>c$

$c > a > b > d$

answer is C.

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Detailed Solution

$Rate law R = K [conc.]^{n} [n \to order] \log (Rate) = logK + nlog [conc.] For \log (rate) v / slog [conc.]graph [Slope = n] As slope increases order (n) increases ∴ Order d > b > a > C$

Therefore, the correct option is (D).

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