The aim is to work out the ventilation requirements for the Sodium Bisulfite (NaHSO3) storage room to ensure COSHH compliance.
From my understanding, the oxidation of NaHSO3 with air results in the formation of SO2.
The vapor cloud above the bisulfite solution is composed of SO2 and H2O.
Available Data
Temperature : 293 K
Vapor Pressure: 4kPa (H2O + SO2)
SO2 Vapor Pressure: 0.9 kPa
Solution Density: 1280 kg/m3
Spillage Volume: 1 m3
Please let me know if any additional info is required.
Oxidation of sodium bisulphite(NaHSO3) with air should give rise to sodium bisulphate (NaHSO4).
But, if you heat NaHSO3 at a sufficiently high temperature, it may decompose producing sulphur dioxide ( SO2) .
Please check a standard text book of general chemistry.
Ashis Ranjan Bandyopadhyay
Thank you for your reply. From literature, we know that the vapour cloud above Sodium Bisulphite solution is composed of SO2 and H2O. What I want to know is suppose you have a m3 spillage of Sodium Bisulphite in the room, how do I use the vapour pressure information to determine the mass/volume of SO2 that will get get released ?
I used the ideal gas equation to get moles/m3 of SO2 .
PV = nRT
n/V = P/RT
Its the next step I have issue with because we don't know the volume of the gas released to convert moles/m3 to moles.
Would I be able to use the volume of the spillage or the tank volume here ?
- Badges
- Science topic
- Similar topics
- Engineering
- Petroleum Engineering
- Gas