Question

During the purification of iron in a blast furnace, the impurity tetraphosphorus decoxide, P₄O₁₀ (1), reacts with solid calcium oxide to produce molten calcium phosphate or slag. 

Write the balanced equation for this reaction. Include physical states. 

equation: 

If the furnace initially contained 24.9 kg of solid calcium oxide and 13.3 kg P,0,.(1), how many kilograms of calcium phosphate were produced during the purification of the iron? 

mass of calcium phosphate: _______ 

Answer 1

Balanced equation is:

6 CaO(s) + P₄O₁₀(l) ==> 2 Ca₃(PO₄)₂(l)

moles CaO = (24.9 x 1000 g) / 56.0774 g/mol = 444.029145431 moles

moles P₄O₁₀ = (13.3 x 1000 g) / 283.889048 g/mol = 46.8492888109 moles

46.8492888109 moles P₄O₁₀ produces 2 x 46.8492888109 = 93.6985776218 moles phosphate

mass of phosphate = 93.6985776218 mol x 310.176724 g/mol = 29063.1178502 g = 29.06 kg

Answer: 29.1 kg

signment Score: 700/2400 Resources Hint Check Answer Question 9 of 24 > During the purification of iron in a blast furnace, the impurity tetraphosphorus decoxide, P,0,.(1), reacts with solid calcium oxide to produce molten calcium phosphate, or slag. Write the balanced equation for this reaction. Include physical states. equation:( 6 Cao (s) + P2010 (1) ► 2 Ca3(PO4)2 (1) If the furnace initially contained 24.9 kg of solid calcium oxide and 13.3 kg P...(I), how many kilograms of calcium phosphate were produced during the purification of the iron? mass of calcium phosphate: 29.1 about us Careers privacy policy contact us terms of use

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