Question

Which gas, co or n2, is expected to behave more ideally at 10 atm and -50°c?

Answer 1

Carbon monoxide (CO) is expected to behave more ideally than nitrogen (N2) at 10 atm and -50°C because it has a smaller molecular size and lower intermolecular forces, making it closer to an ideal gas under these conditions.

Step-by-step explanation:

Between carbon monoxide (CO) and nitrogen (N2), CO is expected to behave more ideally at 10 atm and -50°C. This prediction is based on the principle that a gas behaves more ideally under conditions where there is less intermolecular interaction and the gas particles are moving faster, which minimizes the effects of molecular volume and intermolecular forces.

At a given temperature, lighter gases and those with less complex molecular structures generally behave more ideally because their particles move faster and have less time to interact with one another. Nitrogen (N2) has a larger molecular size compared to CO, and as such, it will experience more intermolecular forces, particularly under high pressures, like 10 atm. Additionally, CO has a smaller quadrupole moment compared to N2, which can cause less intermolecular attraction. The low temperature of -50°C will also aid in minimizing the kinetic energy of both gases, but overall, CO is expected to adhere more closely to the principles of an ideal gas than N2 at these conditions.

Answer 2

Nitrogen, N2, is expected to behave more ideally at 10 atm and -50°C compared to carbon monoxide, CO.

Step-by-step explanation:

The gas that is expected to behave more ideally at 10 atm and -50°C is nitrogen, N2. The behavior of a gas is determined by its deviation from ideal gas behavior, where an ideal gas follows the ideal gas law perfectly. At high pressures and/or low temperatures, gases tend to deviate from ideal behavior, and the extent of deviation depends on the specific gas. Nitrogen has a smaller deviation from ideal behavior compared to carbon monoxide, CO, under these conditions.