$2Y_{2(g)}+x_{2(g)}2Y{O}_2{x}_{(g)}$

$H_{rxn}^o=-218k\frac{J}{m}ol$ reaction

The reaction is first$-$order with respect to $Y{O}_2$ and first$-$order with respect to $x_2.$

A reaction vessel contains $2\mathrm{.}5$mol of $Y{O}_2$ and $1\mathrm{.}5$mol of $x_2,$ and the temperature

is held constant at $298K.$ If the rate constant for the reaction is $0\mathrm{.}005s^{-1},$ what

is the rate of formation of $Y{O}_{2}x?$