Final answer:
To calculate the mass of neon in the second car tire, if the conditions are the same, the mass will be identical to the first tire which is 80.7 g. Additional information implies changes in internal energy due to pressure and temperature differentials, but complete details for calculations are not provided.
Step-by-step explanation:
The student's question involves calculating the mass of neon (Ne) in a car tire and the total mass of gas in another tire using the Ideal Gas Law. Although the question is incomplete, for a given volume and temperature, if the pressure of two tires is the same, the number of moles of gas they contain will also be the same, according to the formula PV = nRT (where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature). Therefore, if one tire with Ne has a mass of 80.7 g, the mass of Ne in the second tire will be the same, assuming that both tires have the same volume and are at the same pressure and temperature. To calculate the total mass of gas in a car tire containing a different gas, you would need the molar mass of that particular gas and the number of moles (derived from PV=nRT).
In regards to the other part of the question where additional information was given, it pertains to changes in internal energy of a gas and the effect of pressure and temperature changes on a gas. This is calculated using different gas law equations and thermodynamic principles.