X(g)+2Y(g)XYX2(g) \ce{X(g) + 2Y(g) -> XY2(g)}

In order to determine the order of the reaction represented above, the initial rate of formation of XYX2\ce{XY2} is measured using different initial values of [X][\ce{X}] and [Y][\ce{Y}]. The results of the experiment are shown in the table below.

Trial[X][Y]Initial Rate of Formation of XYX2(M s1)10.500.508.0×10321.000.503.2×10231.001.006.4×102 \begin{array}{|c|c|c|c|} \hline \text{Trial} & [\ce{X}] & [\ce{Y}] & \text{Initial Rate of Formation of }\ce{XY2} \\ & & & (M \pu{ s^-1}) \\ \hline 1 & 0.50 & 0.50 & 8.0\times 10^{-3} \\ \hline 2 & 1.00 & 0.50 & 3.2 \times 10^{-2} \\ \hline 3 & 1.00 & 1.00 & 6.4\times 10^{-2} \\ \hline \end{array}

In trial 2 which of the reactants would be consumed more rapidly, and why?