Answer:
P2 = 366 mm Hg
Explanation:
We can use the ideal gas law to solve this problem:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature.
Assuming that the number of moles of gas and the temperature remain constant, we can write:
P1V1 = P2V2
where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.
Substituting the given values into the equation, we get:
P1 = 845 mm Hg
V1 = 4.60 L
V2 = 10.6 L
P2 = P1 * V1 / V2
P2 = 845 mm Hg * 4.60 L / 10.6 L
P2 = 366 mm Hg
Therefore, the pressure when the container is expanded to 10.6 L is 366 mm Hg.