Answer to Question #189865 in General Chemistry for khaled

Question

1.   Calcium phosphate, silicon dioxide, and coke may be heated together in an electric furnace to produce phosphorus, as shown in the following equation:

2 Ca3(PO4)2(s) + 6 SiO2(s) + 10 C(s) → 6 CaSiO3(s) + 10 CO(g) + P4(g)

In this reaction, what mass of calcium phosphate would be needed to make 100.0 g of phosphorus? What mass of calcium silicate would be formed as a by-product

Answer 1

100 g= 45.3592 Kg of Phosphours P4

Molar mass of P4 = 123.90 gm/mol

Number of moles of P4 = 45359.2/123.90 = 366.09 moles

Moles of Ca3(PO4)2 required = 2 × moles of P4 = 2 × 366.09 = 732.19 moles

Molar mass of Ca3(PO4)2 = 310.18 gm/mol

Mass of Ca3(PO4)2 required = 732.19 × 310.18 gm = 227110.6942 gms = 227.110 Kg

Mass in Lbs = 500.69 Lbs

number of moles of CaSiO3 formed = 366.09 × 6 = 2196.54 moles

Molar mass of CaSiO3 = 124.33 gm/mol

Weight of CaSiO3 formed = 2196.54 × 124.33 = 273095.81 gms = 273.095 Kg = 602.07 pounds

number of moles of SiO2 required= 366.09 × 6 = 2196.54 moles

Molar mass of SiO2 = 60.08 gm/mol

Weight of SiO2 required = 2196.54 × 60.08 = 131968.12 gms = 131.968 Kg