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What is the correct graphical representation for the parallel reaction, where substrate $A$ converts into $\mathrm{B}$ with rate constant $K_1$ and same substrate $\mathrm{A}$ converts into $\mathrm{C}$ with rate constant $K_2$ . When $K_2 \ggg K_1$
Option: 1

Option: 2

Option: 3

Option: 4

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In case of parallel reaction, A is a reactant, in forward reaction condition concentration of reactant decreases with time whereas concentration of both the products increases with time.

$\\\text{Rate of formation of }\mathrm{B}=\left[\frac{d[B]}{d t}\right]=K_1[A]\\ \\\text{Rate of formation of} \; \mathrm{C}=\left[\frac{d[C]}{d t}\right]=K_2[A]$

Since as per question $K_2 \ggg K_1$ thus at a particular time concentration of $[\mathrm{C}]>[\mathrm{B}]$

Thus, in concentration $\mathrm{v} / \mathrm{s}$ time curve line with respect to $\text{C}$ lies above $\text{B}$ .

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Shailly goel

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