Question

you do:

1. no₂ and co₂ have a similar molecular weight. which gas would you predict to deviate from an ideal gas? justify your selection.
2. if the volume of a gas is greater than you would expect based on the ideal gas law, the best explanation for this is because the....
3. if the volume of a gas is less that you would expect based on the ideal gas law, the best explanation for this is because the....
4. choose a set of conditions (high/low) for each of the following:

most ideal

least ideal

Explanation:

Step1: Analyze gas behavior

Gases deviate from ideal behavior due to intermolecular forces and molecular volume. $\ce{NO2}$ has stronger intermolecular forces (due to its structure and potential for more complex interactions like dimerization in some cases) compared to $\ce{CO2}$ (which has a linear, more symmetric structure and weaker intermolecular forces).

Step2: Justify based on ideal gas assumptions

Ideal gas law assumes no intermolecular forces and negligible molecular volume. $\ce{NO2}$ violates the no - intermolecular - forces assumption more than $\ce{CO2}$ because of its higher tendency for intermolecular attractions.

Answer:

$\ce{NO2}$ would be predicted to deviate more from an ideal gas. This is because $\ce{NO2}$ has stronger intermolecular forces (such as dipole - dipole interactions and potential for more complex associations) compared to $\ce{CO2}$ (which has weaker London dispersion forces as its main intermolecular force due to its linear and more symmetric structure).