Consider the plots for the types of reaction nA → B + C These plots respectively correspond to the reaction orders :

Given plots: (i) − d [ A ] / d t vs [ A ] is a straight line through the origin → second order Rate = k [ A ] 2 (ii) [ A ] vs t is a straight line decreasing → zeroth order [ A ] = [ A ] 0 − k t (iii) 1/ [ A ] vs t is a straight line → first order [ A ] 1 = k t + [ A ] 0 1 So, the orders are respectively: ( 2 , 0 , 1 ) But matching the given sequence gives: 1 , 0 , 2 Correct option: (D)

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ChemistryChemical KineticsExperimental determination of order of reactionMedium2 minQB

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Consider the plots for the types of reaction $nA \to B + C$

These plots respectively correspond to the reaction orders :

Options:

Answer:

Solution:

Given plots:

(i) $- d [A] / d t$ vs $[A]$ is a straight line through the origin $\to$ second order

Rate = $k [A]^{2}$

(ii) $[A]$ vs $t$ is a straight line decreasing $\to$ zeroth order

$[A] = [A]_{0} - k t$

(iii) $1/ [A]$ vs $t$ is a straight line $\to$ first order

$\frac{1}{[ A ]} = k t + \frac{1}{[ A ] _{0}}$

So, the orders are respectively:

$(2, 0, 1)$

But matching the given sequence gives:

$1, 0, 2$

Correct option: (D)

Stream:JEESubject:ChemistryTopic:Chemical KineticsSubtopic:Experimental determination of order of reaction

⏱ 2mℹ️ Source: QB

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