Suppose a $500.mL$ flask is filled with $1\mathrm{.}5$mol of $N{O}_2$ and $0\mathrm{.}30$mol of $NO.$ This reaction becomes possible:

$2N{O}_2(g)2NO(g)+O_2(g)$

Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium.

Use $x$ to stand for the unknown change in the molarity of $O_2.$ You can leave out the $M$ symbol for molarity.

$\backslash$table$[[,N{O}_2,NO,O_2$