Question #42130

Two linear thermometers, A and B, have faulty calibrations. Thermometer A reads the freezing and boiling points of water as $10^\circ \text{A}$ and $130^\circ \text{A}$, respectively. Thermometer B reads the same points as $-20^\circ \text{B}$ and $140^\circ \text{B}$, respectively.

$2 \text{ moles}$ of a monatomic ideal gas are initially at a temperature of $106^\circ \text{A}$. $3 \text{ moles}$ of a diatomic ideal gas are initially at a temperature of $-4^\circ \text{B}$. The two gases are mixed in a rigid, adiabatic container of fixed volume $V = 8.314 \text{ m}^3$.

Assuming no chemical reaction occurs, what is the final equilibrium pressure of the gas mixture? (Take the universal gas constant $R = 8.314 \text{ J mol}^{-1} \text{K}^{-1}$ and absolute zero as $-273^\circ \text{C}$.)