Reaction Order and Rate Laws Homework Help | Page 2

the concentration of HCl while we kept the concentration of Na2S2O3 the same. In Part 2 we
varied the concentration of Na2S2O3 while keeping the concentration of HCl the same.
These are experimental data and results will be different from some of the nice, even numbers
you saw on textbook problems. For example, in this experiment you may double the
concentration of a reactant but the reaction rate may increase anywhere from 1.7 times to 2.4
times. This still means an approximate doubling of the reaction rate. On the other hand, if you
double a reactant concentration and the reaction rate increases by 0.7 to 1.3 times that probably
means that the reaction rate multiplier is one (1).
D. Write the rate law for the reaction.
E. Using the rate law, the rate, and the appropriate concentration(s) from one (or more) of your
experiments calculate k.
F. What are the potential errors in this experiment?