Final answer:
The question requires using the ideal gas law and Dalton's Law of Partial Pressures to determine the total pressure of a mixture of N2 and O2 gases when transferred into a smaller tank at a higher temperature. However, with the data given, compression of gases needs to be considered, which complicates the calculation without more details on how the compression is done.
Step-by-step explanation:
The student's question involves the combining of nitrogen (N2) and oxygen (O2) gases into a smaller tank and calculating the resulting total pressure at an increased temperature. This is a classic application of the ideal gas law, combined with Dalton's Law of Partial Pressures.
To solve this, we can first calculate the total number of moles of each gas using the initial conditions provided, using the ideal gas law (PV=nRT). Then, using the combined volume of the tank and the higher temperature, we would calculate the final total pressure exerted by the gases using the same ideal gas law.
Important to note, though, is the fact that the combined volume of the gases before compression is larger than the volume of the container they are being put into. This implies that the gases need to be compressed, which affects the calculation. However, additional information would be needed regarding how the compression affects the temperature and whether the process is isothermal or adiabatic to provide an accurate calculation for the final pressure.