crfranklin2021 crfranklin2021

Today at 2:21 PM
Chemistry

Answered

If a particular ore contains 56.3 % % calcium phosphate, what minimum mass of the ore must be processed to obtain 1.00 kg k g of phosphorus?

Answer :

maacastrobr maacastrobr

Today at 2:25 PM

Answer:

34.44 kg

Explanation:

First we convert 1.00 kg of phosphorus (P) into moles, using its molar mass:

1.00 kg ÷ 32 kg/kmol = 0.03125 kmol P

Then we convert 0.03125 kmoles of P into kmoles of Ca₃(PO₄)₂:

0.03125 kmol P * [tex]\frac{2kmolCa_3(PO_4)_2}{2kmolP}[/tex] = 0.0625 kmol Ca₃(PO₄)₂

Now we calculate the mass of 0.0625 kmoles of Ca₃(PO₄)₂:

0.0625 kmol Ca₃(PO₄)₂ * 310.18 kg/kmol = 19.39 kg

Finally we calculate the required mass of the ore, using the definition of content percentage:

% content = Mass of calcium phosphate / mass of ore * 100 %

56.3 % = 19.39 kg / mass of ore * 100%

Mass of Ore = 34.44 kg

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