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The reaction rate units is usually in the form mol L^-1 s^-1 (the time unit can vary - s, min, hr, etc). The rate constant depends on the order of the reaction. For example, if first order, the rate constant will be s^-1. You can find this by dividing the units of the reaction rate by the unit of the right hand side. In this case, it is first order so the right hand side unit will be mol L^-1.
The unit for the reaction rate is generally mol*L^-1*s^-1 or M*s^-1 for which M is mol*L-1. As for the units for the rate constant, it depends on the order of the reaction. For zero-order reactions, the units are mol*L^-1*s^-1 or M*s^-1 like the reaction rate. For first-order reactions, the units are s^-1. And for second-order reactions, the units are L*mol^-1*s^-1. You can check this by dividing the units of the reaction rate with the units you have on the other side where for instance, as A->products, the reaction rate=k[A]^1 which would be a first-order reaction. Since [A] is measured in mol*L^-1, you can divide those units to the reaction rate units to be left with s^-1 as the units of k. I believe that in the homework problem it asked us to find the units for the rate constant as well. It is problem 15.9?
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