Which of the following statements is NOT true | vedclass

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(D) Step $1$: The rate law is expressed as $	ext{Rate} = k[A]^x[B]^y$. Here, $k$ is the rate constant.Step $2$: $k$ is independent of the initial con

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The greater the value of the rate constant, the slower the reaction.

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(D) Step $1$: The rate law is expressed as $	ext{Rate} = k[A]^x[B]^y$. Here, $k$ is the rate constant.Step $2$: $k$ is independent of the initial concentration of reactants, but it depends on temperature (Arrhenius equation: $k = Ae^{-E_a/RT}$).Step $3$: $A$ larger value of $k$ indicates a faster reaction rate for a given set of concentrations. Therefore, the statement that a greater value of $k$ makes the reaction slower is incorrect.

Which of the following statements is $NOT$ true about the rate constant $k$?

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