Henry?s law is important in environmental chemistry, where it predicts the distribution of pollutants between water and the atmosphere. The hydrocarbon $m-$xylene $(C_8{H}_{10})$ emitted in wastewater streams, for example, can pass into the air, where it is degraded by processes induced by light from the sun.

The Henry? s law constant for $m-$xylene in water at $25C$ is $370$atm, when the following form of the law is used:

$P_{m^{-\text{x}\text{y}\text{l}\text{e}\text{n}\text{e}}}=k_{m^{-\text{x}\text{y}\text{l}\text{e}\text{n}\text{e}}}{x}_{m^{-\text{x}\text{y}\text{l}\text{e}\text{n}\text{e}}}$

Calculate the partial pressure of $m-$xylene vapor in equilibrium with a solution of $1\mathrm{.}37g$ of $m-$xylene per $1370L$ of water. How many $m-$xylene molecules are present in each cubic centimeter of vapor?

$P_{m-\text{x}\text{y}\text{l}\text{e}\text{n}\text{e}}=,$ atm

molecules per cubic centimeter