Question

A 4.25m^3 tank of chlorine sits in a plant where it can be heated to 85°C during the summer months. The tank is initially charged with 400kg of chlorine. What is the pressure (atm) in the tank under these conditions using 1. The Ideal Gas Equation 2. The truncated Virial Equation (truncated after the second virial coefficient) 3. The SRK Equation

Answer 1

The ideal gas equation :

PV= n RT

Now calculate the number of moles of Cl2 gas:

Molar mass of     Cl2: 70.90 g/ mole

Number of moles = 400 kg or 400*1000 g/ molar mass

= 400*1000 g/ 70.90 g/ mole

= 564.17 moles

Here T = 85°C or 358 K

Volume = 4.25m^3 = 4250 L

R= 0.08206 L- atm / Mole -K

PV = n RT

P = n RT/ V

= 564.17 moles * 0.08206 L- atm / Mole –K*358 K /4250 L

= 3.90 atm