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Unknown Gas Variable

The tank has a volume of 438 L and is filled with 0.885 kg of O2, the tank’s pressure at 21 oC is 1.53 atm. If the tank develops a slow leak that is discovered and sealed. The new measured pressure is 1.37 atm. How many grams of O2 remain? 

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Related questions

a steel tank has a volume of 438L and is filled with .885 kg of O2

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)

1. A mix of N2, O2, CO2 and argon gas is contained in a 40.0 L container. The total pressure is 1.80 atm. T = 25.0 degrees C. The partial pressure of O2

is 0.600 atm. How many grams of O2 are present? Assume ideal behavior.

2. A balloon containing N2 gas has volume 4.80 L at a temperature 32.0 oC. The temperature is changed to -28.0 oC while still at a constant pressure of 762 torr. What will be the balloon’s new volume?

3. What is the mole fraction of Argon in a mixture of Ar, Ne and N2 in a 2.70 L flask, when the partial pressures of the gases are: 0.215 atm Ar ; 0.582 atm Ne and 0.203 atm N2? Temperature is 25 degrees C.

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