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This is true! You can see from the equation [A]=-kt+[A]o that the concentration of A changes only as a result of k and time, not because of its own concentration like in the first order equation (that uses ln[A]) or the second order equation (that uses 1/[A]).
It's not necessarily because the first and second order equations start with ln[A] and 1/[A] instead of just [A], those are just mathematical functions that make it easier to understand the other side of the equation. The rate of reaction in first and second reactions depend on the concentration on initial reaction. However, zero order reactions occur at a rate that is constant throughout the reaction. This can occur if there is a catalyst or enzyme present, for example, which controls the speed of the reaction no matter how much reactant is present.
That is correct; a zero order reaction rate does not depend on the concentration of the reactant present, as long as there is some reactant. When integrating the rate law, we get Rate = . Since anything raised to the zero power is 1, we can see that the rate just depends on k.
It is correct. Zero order reaction usually involves a catalyst or enzyme that works at its maximum potential. Increasing concentration cannot increase the rate the catalyst or enzyme works, and therefore zero order reactions do not depend on the concentration.
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