. What amount of phosphorite is needed to completely react with 2.00 kg SiO2 (molar mass: 60.083 g/mol)? B. How much of an initial 2.65-kg SiO2 remains unreacted if 0.750 kg of phosphorite was used up to produce phosphorus? C. What is the maximum amount of P4 (molar mass: 123.896 g/mol) that can be obtained from 5.00 kg of phosphorite? D. If the percent yield of this process is 73.5%, how much phosphorus is collected from 5.00 kg of phosphorite
Phosphorus can be prepared from calcium phosphate by the following reaction:
2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) ➜ 6CaSiO3(s) + P4(s) + 10CO(g)
Phosphorite is a mineral that contains Ca3(PO4)2 (molar mass: 310.174 g/mol) along with other non-phosphorus-containing compounds. The phosphorite used is 68.5% Ca3(PO4)2 by mass.
A. What amount of phosphorite is needed to completely react with 2.00 kg SiO2 (molar mass: 60.083 g/mol)?
B. How much of an initial 2.65-kg SiO2 remains unreacted if 0.750 kg of phosphorite was used up to produce phosphorus?
C. What is the maximum amount of P4 (molar mass: 123.896 g/mol) that can be obtained from 5.00 kg of phosphorite?
D. If the percent yield of this process is 73.5%, how much phosphorus is collected from 5.00 kg of phosphorite?
Step by step
Solved in 7 steps with 7 images
