A tank holds equal amounts of 4 different gases (H2, He, O2, N2) at a pressure of 896 mm Hg. The tank contains 2.00 L. What is the individual pressure of each of these 4 gases?
When you say equal amounts, is that the same number of moles or the same number of grams, or the same volume, or just what?
Ptotal = P1 + P2 + P3 + P4.
If the mols are equal then the pressure of each is equal so 896/4 = ?? mm. Check my thinking.
Thank you for answering. The problem was given to me in the exact way I typed it. I do not know what my instructor meant by amounts. ( My class has had many issues with her, but I digress.) I think I was making the problem harder than it really was. So then the 2.00 L and types of gas are just extraneous information, I guess. OK, i will go with 224 mm/Hg.
To determine the individual pressure of each gas, you need to use Dalton's law of partial pressures. According to this law, the total pressure exerted by a mixture of gases is the sum of the partial pressures of each gas.
To find the individual pressure of each gas in this scenario, we can use the formula:
Partial Pressure of a Gas = Total Pressure × Mole Fraction of the Gas
First, let's calculate the mole fraction of each gas since we know that the tank holds equal amounts of each gas:
Mole Fraction = Moles of the Gas / Total Moles
Since the tank holds equal amounts of each gas, the mole fraction of each gas will be 1/4.
Now, let's calculate the partial pressure of each gas using the formula above:
For H2:
Partial Pressure of H2 = 896 mm Hg × (1/4) = 224 mm Hg
For He:
Partial Pressure of He = 896 mm Hg × (1/4) = 224 mm Hg
For O2:
Partial Pressure of O2 = 896 mm Hg × (1/4) = 224 mm Hg
For N2:
Partial Pressure of N2 = 896 mm Hg × (1/4) = 224 mm Hg
Therefore, the individual pressure of each gas in the tank is 224 mm Hg for H2, He, O2, and N2.