Which of the following is the incorrect equat | vedclass

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(D) For a zero-order reaction,the integrated rate equation is given by $[R] = -Kt + [R]_0$. Rearranging this,we get $Kt = [R]_0 - [R]$,which implies $

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$[R]_0 + [R] = -Kt$

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(D) For a zero-order reaction,the integrated rate equation is given by $[R] = -Kt + [R]_0$. Rearranging this,we get $Kt = [R]_0 - [R]$,which implies $K = \frac{[R]_0 - [R]}{t}$. Also,$-K = \frac{[R] - [R]_0}{t}$ is a valid rearrangement of the same equation. However,the equation $[R]_0 + [R] = -Kt$ is mathematically incorrect as it does not represent the relationship between concentration and time for a zero-order reaction. Therefore,option $D$ is the incorrect equation.

Which of the following is the incorrect equation for the rate constant of a zero-order reaction?

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