So there was a throw away question that wanted us to calculate the difference in $q$ for a two step process vs single step. Went basically like this:
Gas in a container with a massless a piston. When an external pressure $P_1$ is applied, the gas compresses from $V_i$ to $V_1$. When the external pressure is increased to $P_2$, the gas further compresses from $V_1$ to $V_f$ . In a separate experiment with the same initial conditions, a pressure of $P_2$ was applied to the gas, decreasing its volume from $V_i$ to $V_f$ in one step. If the final temperature was the same for both processes, calculate the difference between $q$ for the two-step process and $q$ for the one-step process.
That was simple enough, heat and work are path functions, $\Delta q=\Delta w$, and we were given the values for pressure and volume. Answer submitted, autograder coughs up the points.
Except that "If the final temperature was the same for both processes" bit is bugging me. How the heck is that possible?
Internal energy is a state function, so $\Delta U=\Delta U_1+\Delta U_2$ (one step, two step), which means $$nC(\Delta T)+P_2(\Delta V_1+\Delta V_2)=nC\Delta T_2+P_2\Delta V_2+nC\Delta T_1+P_1\Delta V_1.$$
And since $\Delta q=\Delta w$,
$$nC(\Delta T)-(nC\Delta T_2+nC\Delta T_1)=P_2(\Delta V_1+\Delta V_2)-(P_2\Delta V_2+P_1\Delta V_1),$$
which can't be true if the final temperature is the same, since that would make $\Delta T=\Delta T_1+\Delta T_1$. The left side would be zero, the right side wouldn't be zero and that's a problem.
What the heck am I missing? Or is the question just badly worded?