Problem: 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.)

FREE Expert Solution

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:

83% (225 ratings)
View Complete Written Solution
Problem Details

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.)

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Henry's Law concept. You can view video lessons to learn Henry's Law. Or if you need more Henry's Law practice, you can also practice Henry's Law practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofFish need at least 4 ppm dissolved O2 for survival.What part...as medium difficulty.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Costanza's class at USF.