We’re being asked to determine the partial pressure of O2 at 10°C using the Henry's Law constant of 1.71x10-3 mol/L atm
In order to determine the partial pressure of O2, we have to find the molarity of O2 first using ppm.
Then use the following equation for partial pressure:
Fish need at least 4 ppm dissolved O2 for survival.
What partial pressure of O2 above the water is needed to obtain this concentration at 10 oC? (The Henrys law constant for O2 at this temperature is 1.71 10-3 mol/L atm.)
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