Chemistry - Chemical Kinetics Question with Solution | TestHub

For the reaction $2\text{A}⟶3\text{C}+\text{D}$, the rate of reaction is expressed as the rate of disappearance of reactants divided by their stoichiometric coefficients, which is equal to the rate of appearance of products divided by their stoichiometric coefficients.

$\text{Rate}=-\frac{1}{2}\frac{\text{d}[\text{A}]}{\text{dt}}=+\frac{1}{3}\frac{\text{d}[\text{C}]}{\text{dt}}=+\frac{\text{d}[\text{D}]}{\text{dt}}$

Comparing this with the given options, the correct relationship is $-\frac{1}{2}\frac{\text{d}[\text{A}]}{\text{dt}}=+\frac{1}{3}\frac{\text{d}[\text{C}]}{\text{dt}}$.

Answer: $-\frac{1}{2}\frac{\text{d}[A]}{\text{dt}}=+\frac{1}{3}\frac{\text{d}[C]}{\text{dt}}$