Question

Part #1:

Which of the following would DECREASE the amount of gas dissolved in your tank?

A) Increase the air pressure above the tank

B) Decrease the Temperature

C) Increase the Temperature

Part #2:

At a particular temperature, you determine that in 50.4 L of water, 0.703 grams of N2 gas are dissolved. You measure the pressure above the tank to be 0.771 atm. Assuming the maximum amount of gas has been dissolved, calculate the Henry's Law constant in the units of mol/(L*atm). Assume that there is ONLY nitrogen in the air above the tank.

Part #3:

You determine that at room temperature (25 oC) the Henry’s Law constant of O2 gas is 1.3 * 10-3 mol/(L*atm). If you have a 50.4 L of water in your fish tank, and the air pressure is 0.771 atm in the room, how many grams of O2 gas could be dissolved? (enter the number only, without units)