Final answer:
The question asks for the difference in internal energy of a gas in a car tire at a higher pressure versus atmospheric pressure. It alludes to using the equation U = NKT, which relates to the temperature and not directly to pressure, making the direct calculation impossible without further information or additional steps not provided.
Step-by-step explanation:
The student's question pertains to the internal energy of a gas in a car tire at a certain volume and pressure. According to the ideal gas law and the equation for the internal energy of an ideal gas (U = NKT, where U is the internal energy, N is the number of molecules, K is the Boltzmann constant, and T is the temperature), we can compare the internal energy of the gas at two different pressures.
When the tire's pressure is 2.20×105 Pa, the gas molecules have more kinetic energy than when the gas is at atmospheric pressure (zero gauge pressure). The question assumes that the number of gas molecules and the temperature (T) remain constant, so we do not need to adjust for changes in these variables.
To calculate the additional internal energy at the higher pressure, we can use the equation U = NKT and consider the difference in pressure from atmospheric pressure. However, the relationship between pressure and internal energy is not direct in the equation provided, and in fact, the internal energy of an ideal gas depends on temperature, not pressure. Therefore, we must acknowledge that we cannot directly calculate the answer from the given equation as internal energy and pressure don't share a direct relation in this form.
The question might be seeking an approach that involves a step not provided within the information, potentially such as the conversion of pressure difference to the equivalent change in temperature, while keeping volume constant, to then find the change in internal energy. However, without specific details on temperature or such a conversion, we cannot provide an exact answer.