X + 2Y ---> XY2
In order to determine the order of the reaction represented above, the initial rate of formation of XY2 is measured using different initial values of [X] and [Y]. The results of the experiment are shown in the table below.
Trial 1) [X] M = .5 M, [Y] M = .5 M, Rate of formation = 8.0 x 10^-3 M/s
Trial 2) [X] M = 1.0 M, [Y] M = .5 M, Rate of formation = 3.2 x 10^-2 M/s
Trial 3) [X] M = 1.0 M, [Y] M = 1.0 M, Rate of formation = 6.4 x 10^-2 M/s
In trial 2 which of the reactants would be consumed more rapidly and why?
Answers:
A) X, because the reaction is second order with respect to X.
B) Y, because the reaction is second order with respect to Y.
C) X, because it has a higher molar concentration.
D) Y, because the rate of disappearance will be double that of X.
