A solution is created by dissolving oxygen in water at $20\backslash$deg C$.$ If the concentration of oxygen in the water is $1\mathrm{.}0$ x $10-3$ m$,$ what is the partial pressure $($atm$)$ of the oxygen gas above the solution? Henry's law constant for oxygen at $20\backslash$deg C is $1\mathrm{.}43$ x $10-3$m$/$atm$.$ Enter your answer with no units.

Selected Answer:

$0\mathrm{.}00001716$

Response Feedback:

Henry's law shows the relationship between the maximum concentration of dissolved gas $($solubility$),$ and the partial pressure of the gas above a solution.

In the equation, C is the solubility of the gas, P is the partial pressure of the gas above the solution, and k is Henry's law constant, which is specific to the gas at a particular temperature.

C space equals space k P

$1\mathrm{.}716x{10}^{-5}is$ incorrect