Does my work here look right?

3. One mole of an ideal gas expands adiabatically into a vacuum. Calculate q, delta-e, w, and delta-H for the process.

q= 0 [adiabatic]

w= -Pext(V2-V1)
w= 0

delta-e = w + q
delta-e = 0 + 0 = 0

delta-h= delta-e + P(delta V)
delta-h= 0 + 0 = 0

does this seem right? The problem doesn't give me any information besides the fact that it's adiabatic, a vacuum, and there's one mole of a gas, so I didn't know the volumes or temperature- that's the only thing that's making me believe that everything is 0.

Based on the given information, it seems like you have correctly deduced that all the values (q, ΔE, w, ΔH) for the process would be zero. Let's break it down to understand why:

1. q = 0: The process is described as adiabatic, which means no heat transfer occurs between the system and its surroundings. Consequently, the value of q, which represents heat transfer, is zero.

2. w = 0: In an adiabatic process, no heat exchange occurs, but work can still be done by the gas. However, since the gas expands into a vacuum, there is no external pressure to do work against, resulting in zero work (w = -Pext(V2 - V1)).

3. ΔE = w + q: This equation represents the change in internal energy of the system. Since both q and w are zero, the change in internal energy (ΔE) will also be zero.

4. ΔH = ΔE + PΔV: ΔH represents the change in enthalpy of the system. In this case, since ΔE is zero and there is no pressure difference (ΔP = 0) because the process occurs in a vacuum, the change in enthalpy (ΔH) will also be zero.

Given that the problem doesn't provide any information about volume or temperature, your reasoning and conclusion that all the values are zero seems reasonable. It aligns with the nature of an adiabatic process occurring in a vacuum, where no heat or work is exchanged.