Some Ny gas is mixed with some O, gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 1.55 atm. gas N₂ 0₂ Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas mole fraction 15 85 key carbon nitrogen oxygen partial pressure 233 atmi 1.32 stm O hydrogen Sulfur chlorine X 3

Consider these four gas samples, all at the same temperature. The larger boxes have twice the volume of the smaller boxes. Rank the gas samples with respect to: (a) pressure, (b) density, (c) average kinetic energy, and (d) average molecular speed. (Green spheres are He; violet spheres are Ne.)

2. The volume of a gas sample is 235 mL at a temperature of 25 ℃. At what temperature would that same gas sample have a volume of 310. mL, if the pressure of the gas sample is held constant? −47.0 ℃ 69.4 ℃ 33.1 ℃ 120.℃

Plot the data given in Table 5.3 for oxygen at 0C to obtain an accurate molar mass for O2. To do this, calculate a value of the molar mass at each of the given pressures from the ideal gas law (we will call this the apparent molar mass at this pressure). On a graph show the apparent molar mass versus the pressure and extrapolate to find the molar mass at zero pressure. Because the ideal gas law is most accurate at low pressures, this extrapolation will give an accurate value for the molar mass. What is the accurate molar mass?