Question

he Deacon process uses hydrochloric acid and oxygen from air to produce chlorine gas and

water. Air is fed into the reactor at about 35% excess, and the fractional conversion to chlorine gas

is about 85%. Procurement needs to know how much acid to purchase, and we are thinking about

using 37% w/w HCl (12M), which has an overall density of 1.19kg/L. How many litres of this 37%

w/w HCl should we purchase per week to get 100,000 litres (STP) of Chlorine gas per week

Answer 1

The deacon process for producing chlorine gas

is given below

Chlorine required = 100,000 litres at STP

At STP

T = 273.15 K

P = 1 atm = 1.013×105 Pa

V = 100,000 litres = 100 m3

(PV/RT )= n

n = (1.013×105) (100) /(8.314×273.15) =

4460.65 mol

Moles of chlorine produced = 4460.65 moles

According to stiochiometry amount of oxygen required to form 4460.65 moles chlorine = 4460.65/2 = 2230.325 moles

Fractional conversion = 85%

Oxygen required = 2230.325/0.85 =

2623.911 moles

According to stiochiometry HCl required =

2623.911(2/0.5) = 10495.647 moles HCl

M. W of HCl = 36.5 g/mol

Amount of HCl required = 10495.647(36.5) = 383091.111 g = 383.0911 Kg

The Hcl should be 37 wt% and 12 M concentration

Total mass of 37 wt% HCl solution

383.0911/0.37 = 1035.381 kg

Density of solution = 1.19 Kg/L

Volume of solution required = (1035.381/1.19) = 874.63 Litres

The molarity of solution = 10495.647/874.63 = 12

To get 100000 litres of chlorine per week we need to purchase 874.63 litres of 37% HCl  

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