1. Convert Units

* Temperature (T): 5 degrees Celsius to Kelvin: 5 + 273.15 = 278.15 K

* Pressure (P): 845 mm Hg to atmospheres (atm): 845 mm Hg / 760 mm Hg/atm = 1.112 atm

* Number of molecules (N): To moles (n): 4.0 x 10^22 molecules / 6.022 x 10^23 molecules/mol = 0.0665 mol

2. Ideal Gas Law

The Ideal Gas Law is: PV = nRT

Where:

* P = Pressure (in atm)

* V = Volume (in liters)

* n = Number of moles

* R = Ideal gas constant (0.0821 L·atm/mol·K)

* T = Temperature (in Kelvin)

3. Solve for Volume (V)

Rearrange the Ideal Gas Law to solve for V:

V = (nRT) / P

4. Calculate

V = (0.0665 mol * 0.0821 L·atm/mol·K * 278.15 K) / 1.112 atm

V ≈ 1.37 L

5. Convert to mL

V ≈ 1.37 L * 1000 mL/L ≈ 1370 mL

Therefore, the volume of the container is approximately 1370 mL.