Final answer:
To compare the gas pressure in a one-liter sample of oxygen, nitrogen, and neon, we can use the Ideal Gas Law equation and compare the number of moles for each gas. Therefore, the gas pressure will be greatest for Neon, followed by Nitrogen, and then Oxygen.
Step-by-step explanation:
In order to compare the gas pressure in a one-liter sample of oxygen, nitrogen, and neon, we need to use the Ideal Gas Law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
Since the volume and temperature are the same for each gas, we can compare the pressures by comparing the number of moles. Using the molar mass of each gas, we can calculate the number of moles:
Oxygen: 2.0 g / 32.0 g/mol = 0.0625 mol,
Nitrogen: 2.0 g / 28.0 g/mol = 0.0714 mol,
Neon: 2.0 g / 20.2 g/mol = 0.099 mol.
Therefore, the gas pressure will be greatest for Neon, followed by Nitrogen, and then Oxygen.