a gases of mixture 80.0g of oxygen and 56.0g nitrogen has a total pressure of 18atm the partial pressure of the in the mixture is what?
figure the moles of each gas, and the total moles.
Partial Pressure O2: molesO2/totalmoles * 18
same with the N2
To find the partial pressure of nitrogen in the mixture, we need to know the mole fraction of nitrogen.
Step 1: Calculate the number of moles of oxygen:
Given mass of oxygen = 80.0 g
Molar mass of oxygen (O₂) = 32.00 g/mol
Number of moles of oxygen = mass / molar mass = 80.0 g / 32.00 g/mol = 2.50 mol
Step 2: Calculate the number of moles of nitrogen:
Given mass of nitrogen = 56.0 g
Molar mass of nitrogen (N₂) = 28.02 g/mol
Number of moles of nitrogen = mass / molar mass = 56.0 g / 28.02 g/mol = 2.00 mol
Step 3: Calculate the mole fraction of nitrogen:
Mole fraction of nitrogen = moles of nitrogen / total moles of gas
Total moles of gas = moles of oxygen + moles of nitrogen = 2.50 mol + 2.00 mol = 4.50 mol
Mole fraction of nitrogen = 2.00 mol / 4.50 mol = 0.4444
Step 4: Calculate the partial pressure of nitrogen:
Partial pressure of nitrogen = mole fraction of nitrogen × total pressure
Partial pressure of nitrogen = 0.4444 × 18 atm = 8.00 atm
Therefore, the partial pressure of nitrogen in the mixture is 8.00 atm.
To find the partial pressure of nitrogen in the mixture, we need to use Dalton's Law of Partial Pressures. According to Dalton's Law, the total pressure of a gas mixture is equal to the sum of the partial pressures of each component in the mixture.
Step 1: Calculate the mole fraction of nitrogen (Xn2) in the mixture.
Mole fraction (X) is the ratio of moles of a component to the total moles of all components in the mixture.
Moles of oxygen (nO2) = Mass of oxygen (mO2) / Molar mass of oxygen (MO2)
Molar mass of oxygen (MO2) = 32 g/mol (approximately)
nO2 = 80.0 g / 32 g/mol = 2.5 mol
Moles of nitrogen (nN2) = Mass of nitrogen (mN2) / Molar mass of nitrogen (MN2)
Molar mass of nitrogen (MN2) = 28 g/mol (approximately)
nN2 = 56.0 g / 28 g/mol = 2.0 mol
Total moles of the mixture = nO2 + nN2 = 2.5 mol + 2.0 mol = 4.5 mol
XN2 = nN2 / Total moles of the mixture
= 2.0 mol / 4.5 mol
≈ 0.444
Step 2: Calculate the partial pressure of nitrogen (PN2).
According to Dalton's Law of Partial Pressures, the partial pressure of nitrogen is equal to the mole fraction of nitrogen in the mixture multiplied by the total pressure.
PN2 = XN2 * Total pressure
= 0.444 * 18 atm
≈ 8.0 atm
Therefore, the partial pressure of nitrogen in the mixture is approximately 8.0 atm.