Lconsider the following reaction: ch3br(aq)+oh−(aq)−→−ch3oh(aq)+br−(a q) the rate law for this reaction is first order in ch3br and first order in oh−. when [ch3br] is 5.0×10−3m and [oh−] is 0.050 m, the reaction rate at 298 k is 0.0432m/s. (a) what is the value of the rate constant? (b) what are the units of the rate constant? (c) what would happen to the rate if the concentration of oh− were tripled? (d) what would happen to the rate if the concentration of both reactants were tripled?