Part A) Which of the following statements is true for ideal gases, but is not always...
Part A) Which of the following statements is true for ideal
gases, but is not always true for real gases?
Choose all that apply.
Molecules are in constant random motion.
Pressure is caused by molecule-wall collisions.
The size of the molecules is unimportant compared to the distances between them.
The volume occupied by the molecules is negligible compared to the volume of the container.
Part B) Which of the following statements is true for real
gases?
Choose all that apply.
Attractive forces between molecules cause an increase in pressure
compared to the ideal gas.
Attractive forces between molecules cause a decrease in pressure compared to the ideal gas.
As molecules increase in size, deviations from ideal behavior become more apparent at relatively high pressures.
As attractive forces between molecules increase, deviations from ideal behavior become more apparent at relatively high temperatures.
Part C) Choose the correct term in the brackets:
In general, real gases behave most ideally at (HIGH/LOW)
pressures and (HIGH/LOW) temperatures.
The behavior of real gases can be described using the van der Waals
equation
[P + (n2a/V2)](V-nb) = nRT
The values of a and b are given below for the two real gases
carbon dioxide and xenon.
The gas in which deviations from ideal behavior due to
intermolecular forces are expected to be the
largestis (CARBON DIOXIDE / XENON )
The gas that would be expected to behave least
like an ideal gas at high pressures is (CARBON DIOXIDE /
XENON)
|
gas |
a (L2atm/mol2) |
b (L/mol) |
|
CO2 |
3.59 |
4.27×10-2 |
|
Xe |
4.19 |
5.11×10-2 |
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