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.
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?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Mass Percent Formula concept. You can view video lessons to learn Mass Percent Formula. Or if you need more Mass Percent Formula practice, you can also practice Mass Percent Formula practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Harris' class at UF.