1. The problem statement, all variables and given/known data 1. Calculate the equilibrium dissolved oxygen concentration for each temperature if PO2 = 21% (this means that if atmospheric pressure is 1 atm then O2 pressure is 21% of that) 2. Relevant equations K19.8/RT = Kp PV=nRT 3. The attempt at a solution K19.8/RT = Kp K19.8 = 1.475x10-3 (1.457x10-3)/(8.314x10-3)(273.15+19.8) = Kp 5.982x10-4 = Kp Kp = (O2 (aq)) / (O2 (g)) 5.982x10-4 = (O2 (aq)) / (0.21) 1.256x104 atm = O2 (aq) ICE table: __________________O2 (g)_______O2 (aq) Initial______________0.21_________0 Change___________0.21 -x_______+x Equilibrium_______0.21 -x_______+x 5.982x10-4 = x/(0.21 – x) 5.982x10-4 (0.21 – x) = x 1.256x10-4 - 5.982x10-4 x = x 1.256x10-4 = x + 5.982x10-4 x 1.256x10-4 = 1.000598x 1.255x10-4 = x PV = nRT n/V = P/RT M = 1.255x10-4 atm/(0.0821atm L/mol K) (273.15 + 19.8) M = 5.218x10-6 This doesn't look right to me but I'm not sure what else to try. Thanks for the help!