The normal boiling points of CO and SO2 are -192 degrees C and -10 degrees C, respectively

A) At 25 degrees C and 1 atm, which gas would you expect to have a molar volume closest to the ideal value?
B) If you reduce the deviation from ideal gas behavior, in what direction would you change the temperature? The pressure?

Two questions:
How do you calculate molar volume?
For B), would the pressure stay the same since it's 1 atm and molar volume deviates more as it approaches more extreme temperatures/pressures?

A) PV=nRT
T is the same. R is the same. n is the same. P is the same. Volume is the only variable that can change.
Real gases deviate from ideal behavior most at low temperatures or extremely high pressure. These deviations occur because the volume of the gas is not negligible AND because the attraction between molecules is not negligible. Given that CO and SO2 both have dipole moments, that CO is smaller than SO2, and that SO2 is nearer its liquification temperature than CO, which do you think?
B)Remember to stay away from low T and high P.

To calculate molar volume, use the gas equation, PV = nRT or is that obvious and you had something else in mind.
I don't understand your question under B. Perhaps another tutor will

"To calculate molar volume, use the gas equation, PV = nRT or is that obvious and you had something else in mind."

Well what I'm confused about in this case is that since T, R, and P are the same for both CO2 and SO2, does that mean that the volumes are the same?

For an ideal gas, yes. For a real gas, no. For real gases, look up a and b for each of the gases and use the van der Waals equation of state (unless you are determining all this from an experiment).

The van der Waals equation of state takes into account the attractive forces between molecules and the finite size of the molecules.

In the case of comparing CO and SO2, we can assume that they are behaving as ideal gases at 25 degrees C and 1 atm. In this scenario, the molar volume can be calculated using the ideal gas 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.

Since the given conditions for both CO and SO2 are the same (25 degrees C and 1 atm), the molar volumes of the two gases would be the same if they were ideal gases.

However, since real gases deviate from ideal behavior, the molar volumes of CO and SO2 are not expected to be exactly equal. Based on the properties mentioned, such as the dipole moments, size, and proximity to the liquification temperature, it is likely that CO would have a molar volume closest to the ideal value at 25 degrees C and 1 atm.

Regarding your question about reducing the deviation from ideal gas behavior, temperature and pressure can be adjusted. To minimize the deviations, it is advisable to stay away from low temperatures and high pressures.

In this case, if you want to reduce the deviation, you would need to increase the temperature and/or decrease the pressure. This is because deviations from ideal gas behavior are more pronounced at low temperatures and high pressures. By increasing the temperature or decreasing the pressure, you would be moving the system away from these extreme conditions, leading to a reduction in deviation from ideal gas behavior.

Regarding your question about the pressure staying the same since it's 1 atm, it is worth noting that pressure is one of the variables that can be adjusted to reduce the deviation from ideal gas behavior. While the pressure is given as 1 atm in this scenario, it can still be altered if necessary to minimize deviations from ideal behavior.

The van der Waals equation of state is given by:

(P + a/V^2)(V - b) = nRT

Where P is the pressure, V is the molar volume, n is the number of moles, R is the ideal gas constant, T is the temperature, a and b are the van der Waals constants specific to each gas.

The van der Waals equation takes into account the fact that real gases have finite volumes and attractive forces between the gas molecules. The term a/V^2 accounts for the attractive forces, and the term -b accounts for the volume occupied by the gas molecules.

Since the pressure (P) and temperature (T) are the same for both CO and SO2, the molar volume (V) can be used to compare which gas is closest to the ideal behavior. Generally, gases deviate from ideal behavior more at low temperatures or high pressures where the volume of the gas and the attractive forces between molecules are not negligible.

In this case, we can compare the molar volumes of CO and SO2. CO is smaller than SO2 and is farther from its liquefaction temperature compared to SO2. This means that the volume occupied by CO is relatively less and the attractive forces between CO molecules are relatively weaker compared to SO2. Therefore, CO would be expected to have a molar volume closer to the ideal value at 25 degrees C and 1 atm.

For question B, reducing the deviation from ideal gas behavior means making the molar volume closer to the ideal value. To achieve this, since the pressure is already fixed at 1 atm in this case, you would need to change the temperature. Generally, at lower temperatures and higher pressures, real gases deviate more from ideal behavior. So, to reduce the deviation, you would increase the temperature and decrease the pressure. However, in this specific case, since the pressure is already at 1 atm, you would focus on changing the temperature away from extreme low temperatures.

I hope this answers your questions!