Question # $4.$

A $0\mathrm{.}25-L$ glass of water is in equilibrium with air at $0C$ and contains $8\mathrm{.}19{10}^{-4}$mol$\%$ oxygen. The glass is brought to a room at $20C.$ How much oxygen $($in $g)$ will be released from the glass to reach equilibrium at $20C?$ Air is assumed to be mixture of oxygen $(O_2)$ and nitrogen only $(N_2).$ Data at $20C$ : Henry's constant of oxygen in water is $40,100$atm. The vapor pressure of water at $20C$ is $0\mathrm{.}023$atm, and the mole ratio of oxygen and nitrogen in the equilibrium air above the glass of water is $0\mathrm{.}21$:$0\mathrm{.}79.$ The molar volume of equilibrium water in glass is approximately $0\mathrm{.}018L.$ Molar mass of oxygen $=32k\frac{g}{k}$mol

$V_L=0\mathrm{.}25L$

$T_i=0C,T_z=20C$

$8\mathrm{.}19{10}^{-4}$mol$\%$ oxygen $H_i=40100$atm

$M=32k\frac{g}{k}molO{z}_2$