In order to determine the order of the reaction represented above, the initial rate of formation of XYX2 is measured
using different initial values of [X] and [Y]. The results of the experiment are shown in the table below.
Trial123[X]0.501.001.00[Y]0.500.501.00Initial Rate of Formation of XYX2(Ms−1)8.0×10−33.2×10−26.4×10−2
In trial 2 which of the reactants would be consumed more rapidly, and why?
Approach
Using the method of initial rates, we could confirm that the reaction is second order with respect to X and first order with respect to Y.
Using that method is timely and unncessary. We can simply look at the stoichiometric ratios of the balanced reaction.
2 molecules of Y are consumed for every molecule of X. Therefore, Y will be consumed more rapidly.