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10 March, 07:49

If a particular ore contains 55.4% calcium phosphate, what minimum mass of the ore must be processed to obtain 1.00kg of phosphorus?

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  1. 10 March, 11:14
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    First, we require the formula of calcium phosphate. This is:

    Ca₃ (PO₄) ₂

    And its mass is 310 g/mol

    The atomic mass of phosphorus is 31 g/mol, and as there are 2 moles of P per mole of calcium phosphate, the mass of P is 62 g / mol calcium phosphate

    Now, we calculate the percentage mass of phosphorus in calcium phosphate. This is:

    62/310 * 100 = 20%

    So, if we need 1 kg of P, we need:

    1/20% = 5 kg of calcium phosphate. This means we need:

    5 / 55.4% = 9.02 kg of ore

    9.02 kg of ore is required.
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