The reaction A + B —–> C + D has an initial rate of 0.0790 M/s.
rate = k [A] [B] ^2
a) What will the initial rate (in m/s ) be if [A] is halved and [B] is tripled?
b) What will the initial rate (in m/s ) be if [A] is tripled and [B] is halved?
When the initial concentrations of the reactants are changed by any factor, then the first step is to write the new concentrations in terms of the initial concentrations. Then, write the new rate law in terms of the initial concentrations. And then calculate the new rate law by substituting the values accordingly.