Molecular size in real gases causes positive deviations from the PV/RT ratio of an ideal gas.
a. True
b. False
as temp goes to absolute zero, theory would state V goes to zero. But the actual size of molecules prevents V from becoming zero.
true
true
a. True
Explanation:
In real gases, the individual molecules have a finite size and a certain amount of intermolecular interactions. These interactions cause the molecules to take up space and exert forces on each other. As a result, the actual volume occupied by the gas molecules is greater than the idealized volume of an ideal gas.
This increase in volume leads to an increase in the overall pressure of the gas, which in turn causes a positive deviation from the ideal gas law equation PV = nRT.
Hence, due to the molecular size and intermolecular interactions, real gases deviate from the ideal gas behavior, resulting in positive deviations from the PV/RT ratio of an ideal gas.