Ask Question
24 January, 20:14

If a particular ore contains 58.3 % calcium phosphate, what minimum mass of the ore must be processed to obtain 1.00 kg of phosphorus?

+5
Answers (1)
  1. 24 January, 21:59
    0
    Molecular formula of calcium phosphate: Ca3 [PO4]2

    Molar mass of calcium phosphate: 3*40.1g/mol + 2*31.0 g/mol + 2*4*16.0 g/mol = 310.3 g/mol

    Mass of phosphorus in the molecular formula: 2*31.0 g/mol = 62.0 g/mol

    Ratios:

    x * 0.583 g of calcium phosphate / g of ore * 62.0 g of phosphorus / 310.3 g of calcium phosphate = 1000 g of phosphorus

    0.11649 x g of phospuros / g of ore = 1000 g of phosphorus

    x = 1000 g of phosphorus / 0.11649 g of phosphorus / g of ore

    x = 8585 g of ore = 8.585 kg of ore
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “If a particular ore contains 58.3 % calcium phosphate, what minimum mass of the ore must be processed to obtain 1.00 kg of phosphorus? ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers