Question

What is the unit of rate constant for a zero-order reaction?

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Solution

Rate constantThe equation for rate is as follows:- $\text{Rate}=k{\left[\text{A}\right]}^{\mathrm{x}}{\left[B\right]}^{\mathrm{y}}......\left(1\right)\phantom{\rule{0ex}{0ex}}-\frac{d\left[\text{R}\right]}{dt}=k{\left[\text{A}\right]}^{\mathrm{x}}{\left[B\right]}^{\mathrm{y}}....\left(2\right)$This form of equation (2) is known as the differential rate equation. Here, k is the rate constant.Unit of rate constant for zero-order$k=\frac{\text{Rate}}{{\left[A\right]}^{\mathrm{x}}{\left[B\right]}^{\mathrm{y}}}\phantom{\rule{0ex}{0ex}}=\frac{\text{Concentration}}{\text{Time}}×\frac{1}{{\left[\text{Concentration}\right]}^{\mathrm{n}}}\phantom{\rule{0ex}{0ex}}=\frac{{\text{molL}}^{-1}}{\text{s}}×\frac{1}{{\left[{\text{molL}}^{-1}\right]}^{0}}\phantom{\rule{0ex}{0ex}}={\text{molL}}^{-1}{\text{s}}^{\text{-1}}$Here, n is the order of the reaction.So, the unit of rate constant for zero-order is ${\text{molL}}^{\text{-1}}{\text{s}}^{\text{-1}}$.

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