Anhydrous ferrous sulfate (FeSO4) crystals are produced from an aqueous solution in a two step process. A solution of 0.256 mass fraction of FeSO4 and 0.744 mass fraction H2O at 41.1°C enters a crystallizer. Within the crystallizer, the temperature drops to 7.86°C, producing iron (II) sulfate heptahydrate (FeSO4·7H2O) crystals and an aqueous FeSO4 solution. The FeSO4·7H2O crystals are sent through a dryer that produces anhydrous FeSO4 and water. If the facility wishes to produce 27.6 pounds of anhydrous FeSO4 per hour, what are the mass flow rates of the aqueous FeSO4 solutions entering and leaving the crystallizer, and what is the composition of the aqueous solution leaving the crystallizer? For the temperature ranges described, the solubility of FeSO4 in water is described by: y = 0.6578T 14.282 where T is the temperature of the solution in °C and y is the solubility of FeSO4 in g FeSO4/100 g H2O
1.What is the solubility of FeSO4 in water at 7.86°C?
2.What are the mass fractions of FeSO4 and H2O in the aqueous stream leaving the crystallizer?
3.What is m4, the mass flow rate of water from the dryer? What is m1, the mass flow rate of aqueous FeSO4 solution entering the crystallizer??
4.What is m2, the mass flow rate of the aqueous FeSO4 solution leaving the crystallizer?