Question

What quantity in moles of chlorine gas at 120.0°C and 33.3 atm would occupy a vessel of 18.5 L? Options: Option 1: 0.833 moles Option 2: 2.008 moles Option 3: 4.287 moles Option 4: 6.119 moles

Answer 1

Using the Ideal Gas Law, the quantity of chlorine gas that would occupy 18.5 L at 120.0°C and 33.3 atm is calculated to be approximately 2.008 moles, which corresponds to Option 2.

Step-by-step explanation:

To determine the quantity in moles of chlorine gas that would occupy a volume of 18.5 L at 120.0°C and 33.3 atm, we can use the Ideal Gas Law, which is stated as PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the universal gas constant, and T is the temperature in Kelvin.

First, convert the temperature to Kelvin:
120.0°C + 273.15 = 393.15 K

Next, use the Ideal Gas Law to solve for n (moles of Cl2):

(33.3 atm) × (18.5 L) = n × (0.0821 L·atm/K·mol) × (393.15 K)
n = [(33.3) × (18.5)] / [(0.0821) × (393.15)]
n ≈ 2.008 moles

Thus, the correct answer is Option 2: 2.008 moles of chlorine gas.