a 12.5 g sample of oxygen gas is added to a 25.og sample of nitrogen gas in a 25.0L'Container at 28 C. Calculate the partial pressure of each gas and the total pressure of he mixture. answer
mols O2 = grams/molar mass.
mols N2 = grams/molar mass.
PV = nRT, use n for each gas and solve for P. Don't forget T must be in kelvin.
Then total P = pO2 + pN2.
To calculate the partial pressure of each gas and the total pressure of the mixture, we will need to use the Ideal Gas Law and Dalton's Law of Partial Pressures.
First, let's calculate the number of moles for each gas using their respective masses and molar masses.
The molar mass of oxygen (O2) is approximately 32 g/mol, and the molar mass of nitrogen (N2) is approximately 28 g/mol.
For oxygen:
Number of moles = mass / molar mass
Number of moles of O2 = 12.5 g / 32 g/mol
Number of moles of O2 = 0.39 mol
For nitrogen:
Number of moles = mass / molar mass
Number of moles of N2 = 25.0 g / 28 g/mol
Number of moles of N2 = 0.89 mol
Next, let's use the Ideal Gas Law equation (PV = nRT) to calculate the partial pressures of each gas. Since the temperature is given in Celsius, we need to convert it to Kelvin by adding 273.15.
The Ideal Gas Law equation can be rearranged as P = (nRT) / V, where P represents pressure, n represents the number of moles, R is the ideal gas constant (0.0821 L∙atm/mol∙K), T is the temperature in Kelvin, and V is the volume.
For oxygen:
P(O2) = (n(O2) * R * T) / V
P(O2) = (0.39 mol * 0.0821 L∙atm/mol∙K * (28 + 273.15) K) / 25.0 L
P(O2) = 0.962 atm
For nitrogen:
P(N2) = (n(N2) * R * T) / V
P(N2) = (0.89 mol * 0.0821 L∙atm/mol∙K * (28 + 273.15) K) / 25.0 L
P(N2) = 2.47 atm
Finally, to calculate the total pressure of the mixture, we can simply add the partial pressures of both gases.
Total pressure = P(O2) + P(N2)
Total pressure = 0.962 atm + 2.47 atm
Total pressure = 3.432 atm
Therefore, the partial pressure of oxygen gas is 0.962 atm, the partial pressure of nitrogen gas is 2.47 atm, and the total pressure of the mixture is 3.432 atm.