Air at $1$ bar pressure containing $1$mol$\%$ of methane $,$ molecular weight $\{$:$16\mathrm{.}0\frac{g}{m}ol)$ comes

into contact and equilibrates with a $1L$ glass of water at a temperature of $25C.$ Assume ideal

solution behavior throughout this problem.

a$.$ How much methane $($in milligrams$)$ is dissolved in the water at $25C?$

b$.$ Suppose I drink the water, adding the $1L$ to the $40L$ of fluid $($treat as all water$)$ in my

body. What is the mole fraction of methane in my body?

c$.$ Now the methane and water are at $37C$ in my body. What is the equilibrium vapor

pressure of methane under these conditions? This is what would be expected to be

expelled in my breath.