   Chapter 2, Problem 138GQ

Chapter
Section
Textbook Problem

Elemental phosphorus is made by heating calcium phosphate with carbon and sand in an electric furnace. What is the mass percent of phosphorus in calcium phosphate? Use this value to calculate the mass of calcium phosphate (in kilograms) that must be used to produce 15.0 kg of phosphorus.

Interpretation Introduction

Interpretation: The mass percent of phosphorus in calcium phosphate and the mass of calcium phosphate that must be used to produce 15.0kg of phosphorus should be determined.

Concept introduction:

• Moleofsubstance=GramofsubstanceMolarmass
• The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol)
• Mass percentage is one way to represent the concentration of an element in a compound or a component in a mixture. Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.
Explanation

Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.

The molecular formula of calcium phosphate is Ca3(PO4)2

Then, the mass percent of phosphorus in calcium phosphate can be calculated as follows,

Molar mass of phosphorus in the compound is 2×30.974=61.95g/mol

MasspercentofphosphorusinCa3(PO4)2=MolarmassofphosphorusMolarmassofCa3(PO4)2×100 =61

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 