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WorksheetsIdeal Behavior
Total questions: 10
Worksheet time: 11mins
Under what conditions do real gases behave most like an ideal gas?
Low temperature and low pressure
Low temperature and high pressure
High temperature and low pressure
High temperature and high pressure
What gases deviate most from ideal behavior?
polar molecules with small molar masses
polar molecules with large molar masses
nonpolar molecules with small molar masses
nonpolar molecules with large molar masses
Which of the following behaves most like an ideal gas at the conditions indicated?
H2(g) molecules at 10-3 atm and 200°C
O2(g) molecules at 20 atm and 200°C
SO2(g) molecules at 20 atm and 200°C
NH3(g) molecules at 20 atm and 200°C
NH3(g) molecules at 20 atm and 300°C
The table below contains information about samples of four different gases at 273 K. The samples are in four identical rigid containers numbered 1 through 4.
The best explanation for the lower pressure in container 4 is that SO2 molecules
have a larger average speed than the other three gases
occupy a larger portion of the container volume than the other three gases
have stronger intermolecular attractions than the other three gases
contain 𝜋 bonds, while the other gases contain σ only bonds
Ar(g) deviates more from ideal behavior at extremely high pressures than Ne(g) does. Which of the following is one reason for this difference?
The particle volume of Ar is greater than that of Ne.
Ar atoms have more valence electrons than Ne atoms have, so atoms have greater interparticle forces.
The intermolecular forces between Ne atoms are greater than those between Ar atoms.
Ar atoms are more attracted to the walls of the container than Ne atoms are.
Under which of the following conditions of temperature and pressure will H2 gas be expected to behave most like an ideal gas?
50 K and 0.10 atm
50 K and 5.0 atm
500 K and 0.10 atm
500 K and 50 atm
Which of the following best helps explain why the pressure of a sample of CH4 (molar mass 16 g/mol) is closer to the pressure predicted by the ideal gas law than a sample of NH3 (molar mass 17 g/mol)?
NH3 molecules are polar while CH4 molecules are not, and the greater attractions between NH3 molecules cause the molecules to collide with the walls of the container with less force.
NH3 molecules have a greater molar mass than CH4 molecules, so the NH3 molecules collide with the walls of the container with more force.
CH4 molecules have more hydrogen atoms than NH3 molecules, so CH4 molecules have more hydrogen bonding and greater intermolecular forces.
CH4 molecules are larger than NH3 molecules, so the actual CH4 molecules take up a significant portion of the volume of the gas.
The diagrams above represent two samples of Xe gas in containers of equal volume at 280 K. Which of the following correctly compares the two samples in terms of their deviation from ideal gas behavior and explains why?
The gas in sample 1 would deviate more from ideal behavior because the average distance an Xe atom travels before colliding with another Xe atom is greater.
The gas in sample 2 would deviate more from ideal behavior because the Xe atoms are closer together, leading to an increase in intermolecular attractions.
The gas in sample 2 would deviate more from ideal behavior because the average speed of the Xe atoms is less, leading to an increase in intermolecular attractions.
The gases in both sample 1 and sample 2 would show the same deviation from ideal behavior.
A vessel contains Ar(g) at a high pressure. Which of the following statements best helps to explain why the measured pressure is significantly greater than the pressure calculated using the ideal gas law?
The molar mass of Ar is relatively large.
A significant number of Ar2 molecules form.
The attractive forces among Ar atoms cause them to collide with the walls of the container with less force.
The combined volume of the Ar atoms is too large to be negligible compared with the total volume of the container.
Which gas deviates most from ideal behavior?
SO2
Ne
CH4
N2
H2
