A gaseous mixture of O2 and N2 contains 32.8% nitrogen by mass
How do i figure out wat the mass is?
Mass of what? I don't think there is enough information to determine the mass of either oxygen or nitrogen. You know, of course, that percent oxygen = 100-32.8.
oh sry, didn't the whole question
A gaseous mixture of O2 and N2 contains 32.8% nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 665mmHg ?
would i start by calculating the number of moles of nitrogen? if so how?
Have you had anything about mole fractions? There may be a short way of solving this problem but I would suggest the following, although it is long.
I would assume a mass of total gas of some number. Then 67.2% of that number and 32.8% of that number will give you grams of N2 and grams O2. Then convert each to mols, determine mole fraction from that, then partial pressure = mole fraction x 665 to give pressure of each.
To determine the mass of the gaseous mixture, you first need to know the total mass of the mixture. However, since the question does not provide the mass of the mixture, we cannot calculate it directly.
If you are given additional information, such as the total pressure, temperature, or volume of the mixture, you can use the ideal gas law to calculate the mass. The ideal gas law states that:
PV = nRT
Where:
P = pressure of the gas
V = volume of the gas
n = number of moles of gas
R = ideal gas constant
T = temperature in Kelvin
If you know the pressure, volume, and temperature, you can calculate the number of moles (n) using the ideal gas law. Then, you can multiply the number of moles by the molar mass of the gaseous mixture to obtain the mass.
However, if the information provided in the question is limited to only the percentage of nitrogen by mass, it is not possible to calculate the mass of the mixture without additional information.