For a hypothetical reaction: A + 2B + C → D + E The rate law has been determined and is as follows: Rate = k[A][B]2 What happens to the reaction rate when we make each of the following concentration changes? a)  We triple the concentration of A without changing the concentration of B or C. b)  We triple the concentration of B without changing the concentration of A or C. c)  We triple the concentration of C without changing the concentration of A or B. d)  We triple the concentrations of A, B and C simultaneously. e)  We triple the concentration of D.

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