For a gas sample whose total pressure is 740 torr, what are the partial pressures if the moles of gas present are 1.3 mol N2, 0.33 mol O2, and 0.061 mol Ar?
Calculate mols fraction each gas.
For example, XN2 = (mols N2/total mols)
Do the same for XO2 and XAr
Then peach = Xeach*Ptotal
To determine the partial pressures of the gases in the sample, we need to use Dalton's Law of Partial Pressures. According to this law, the total pressure of a mixture of non-reacting gases is equal to the sum of the partial pressures of each gas.
The partial pressure of each gas can be calculated using the formula:
Partial Pressure = (Moles of Gas / Total Moles of Gas) × Total Pressure
1. First, find the total moles of gas by adding up the moles of each gas:
Total Moles of Gas = 1.3 mol N2 + 0.33 mol O2 + 0.061 mol Ar
2. Calculate the partial pressure of each gas using the formula mentioned above:
Partial Pressure of N2 = (1.3 mol N2 / Total Moles of Gas) × 740 torr
Partial Pressure of O2 = (0.33 mol O2 / Total Moles of Gas) × 740 torr
Partial Pressure of Ar = (0.061 mol Ar / Total Moles of Gas) × 740 torr
3. Substitute the values and calculate:
Partial Pressure of N2 = (1.3 mol N2 / (1.3 mol N2 + 0.33 mol O2 + 0.061 mol Ar)) × 740 torr
Partial Pressure of O2 = (0.33 mol O2 / (1.3 mol N2 + 0.33 mol O2 + 0.061 mol Ar)) × 740 torr
Partial Pressure of Ar = (0.061 mol Ar / (1.3 mol N2 + 0.33 mol O2 + 0.061 mol Ar)) × 740 torr
These calculations will give you the partial pressures of N2, O2, and Ar in the gas sample.
To determine the partial pressures of each gas in the sample, you can use Dalton's Law of Partial Pressures, which states that the total pressure of a mixture of non-reacting gases is equal to the sum of their individual partial pressures.
1. First, calculate the total moles of gas in the sample:
Total moles of gas = moles of N2 + moles of O2 + moles of Ar
Total moles of gas = 1.3 mol + 0.33 mol + 0.061 mol = 1.691 mol
2. Next, calculate the mole fraction of each gas. Mole fraction is the ratio of the moles of a specific gas to the total moles of gas in the sample.
Mole fraction of N2 = moles of N2 / total moles of gas
Mole fraction of N2 = 1.3 mol / 1.691 mol ≈ 0.768
Similarly, calculate the mole fractions of O2 and Ar:
Mole fraction of O2 = 0.33 mol / 1.691 mol ≈ 0.195
Mole fraction of Ar = 0.061 mol / 1.691 mol ≈ 0.036
3. Now, use the mole fractions to calculate the partial pressures of each gas. Multiply the mole fraction of each gas by the total pressure of the sample.
Partial pressure of N2 = Mole fraction of N2 * Total pressure
Partial pressure of N2 = 0.768 * 740 torr ≈ 568.32 torr
Partial pressure of O2 = Mole fraction of O2 * Total pressure
Partial pressure of O2 = 0.195 * 740 torr ≈ 144.3 torr
Partial pressure of Ar = Mole fraction of Ar * Total pressure
Partial pressure of Ar = 0.036 * 740 torr ≈ 26.64 torr
Therefore, the partial pressures of N2, O2, and Ar in the gas sample are approximately 568.32 torr, 144.3 torr, and 26.64 torr respectively.