Problem: Phosphorus is obtained primarily from ores containing calcium phosphate.If a particular ore contains 57.1 % calcium phosphate, what minimum mass of the ore must be processed to obtain 1.00 kg of phosphorus?

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We are asked to determine the minimum mass of the ore containing calcium phosphate (Ca3(PO4)2) that must be processed to obtain 1.00 kg of phosphorus (P)

To solve this problem, we shall follow these steps:

Step 1: Convert grams to moles of phosphorus using the molar mass of phosphorus.

Step 2: Perform a mole-to-mole comparison between phosphorus(P) and calcium phosphate (Ca3(PO4)2), 2 mol P: 1 mol Ca3(PO4)2.

Step 3: Compute for the mass of calcium phosphate (Ca3(PO4)2) using the obtained moles of calcium phosphate and the molar mass of calcium phosphate (Ca3(PO4)2). 

Step 4: Convert the mass from g to kg. Take into account the percentage given in the problem to determine the number of kilograms of the ore that is required.

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Problem Details

Phosphorus is obtained primarily from ores containing calcium phosphate.

If a particular ore contains 57.1 % calcium phosphate, what minimum mass of the ore must be processed to obtain 1.00 kg of phosphorus?