An ideal gas differs from a real gas in that the molecules of an ideal gas:
have no kinetic energy
have a molecular weight of zero
have no attraction for one another
have appreciable molecular volumes
have an average molecular mass
I believe the answer is "have no attraction for one another," am I correct?
yes
Yes, you are correct. An ideal gas differs from a real gas in that the molecules of an ideal gas have no attraction for one another. In an ideal gas, the molecules are assumed to have no intermolecular forces acting between them, which means they do not interact or exert any attractive or repulsive forces on each other. This assumption simplifies the mathematical calculations involved in studying the behavior of gases and allows for the use of the ideal gas law.
Yes, you are correct. An ideal gas differs from a real gas in that its molecules have no attraction for one another. To understand why this is the correct answer, let's break down each of the options:
1. "Have no kinetic energy": This option is not correct because all gases, whether ideal or real, have molecules in constant motion, which is characterized by kinetic energy.
2. "Have a molecular weight of zero": This option is not correct because molecules of both ideal and real gases have finite molecular weights. The molecular weight represents the mass of one molecule of the gas.
3. "Have no attraction for one another": This option is correct. In an ideal gas, the molecules are considered to have no attractive forces between them. This assumption simplifies calculations and allows for easier analysis.
4. "Have appreciable molecular volumes": This option is not correct because ideal gas molecules are assumed to have negligible molecular volumes. In other words, the volume of the gas molecules themselves is considered to be insignificant compared to the total volume occupied by the gas.
5. "Have an average molecular mass": This option is not correct because both ideal and real gases have an average molecular mass. The average molecular mass of a gas is calculated based on the individual masses and abundances of its different molecules.
Therefore, the correct option is "have no attraction for one another" when considering how ideal gases differ from real gases.