Answer:
The statements to examine are missing, but check the explanation to obtain a clear understanding of the question and the subject matter.
Explanation:
Ideal gases have properties such that
- The gas molecules occupy a negligible volume compared to the volume occupied by the gas.
- The gas molecules are largely identical.
- The gas molecules are in a constant state of random motion, collide with each other and the walls of the containing container elastically and obey the laws of elastic collision. Basically, they obey the kinetic theory of gases.
- The forces of attraction between ideal gas molecules are negligible.
But real gases deviate from ideal behaviour because their molecules occupy considerable volume and there exists forces of attraction among them. Completely ideal behaviour is theoretical because of these reasons.
At low pressure and high temperature, real gases behave approximately as ideal gases.
Methane gas has relatively large molecules, and the intermolecular forces are much larger than required for an ideal gas. Hence, it is a gas that deviates from idealness.
Ethane is farther from being an ideal gas. It suffers from the same properties as methane, only more so. It has even larger molecules and a stronger intermolecular force of attraction due to the presence of double bonds in its structure. This seriously interferes with the state of random motion expected for ideal gases.
Hope this Helps!!!
Answer:
C₂H₆ molecules have a larger, more polarizable electron cloud than CH₄ molecules do.
Explanation:
There are greater attractive forces among ethane molecules. They pull the molecules closer together, and the gas occupies less volume.
For example, the molar volume of an ideal gas at STP — 0 °C and 1 bar — is 22.71 L.
Under the same conditions the molar volume of methane is 22.65 L, and that of ethane is 22.53 L.
