If a particular ore contains 58.5% calcium phosphate, what minimum mass of the ore must be processed to obtain 1.00 kg of phosphorus?

The minimum mass of the ore is .

Further explanation:

Molar mass:

The molar mass of a compound is the summation of masses of all atoms or molecules present in the 1 mole of compound. In other words, Molar mass of a compound is the ratio of the mass of compound in grams to the number of moles present of that compound. The S.I unit of molar mass is gram per mol or g/mol.

The molar mass of   is calculated as follows:

                  …… (1)

The atomic mass of Ca is 40 g.

The atomic mass of P is 30.974 g.

The atomic mass of O is 16 g.

Substitute these values in equation (1).

The percentage of P in is calculated as follows:

                       …… (2)

The atomic mass of P is 30.974 g.

The atomic mass of is 309.948 g/mol.

Substitute these values in equation (2).

The mass of phosphorus is converted to g. The conversion factor for this is,

So the mass of phosphorus is calculated as follows:

The amount of  is calculated as follows:

                      …… (3)

Substitute 1000 g for the mass of P and 10 % for % of P in equation (2).

The mass of ore can be calculated as follows:

                     …… (4)

Substitute 10000 g for the mass of  and 58.5 % for % of   in equation (4).

So the minimum mass of the ore is 17094 g.

Learn more:

1. Calculate the moles of chlorine in 8 moles of carbon tetrachloride:

2. Calculate the moles of ions in the solution:

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Mole concept

Keywords: molar mass, P, atomic mass, 10 %, 58.5 %, 17094 g, ore, Ca3(PO4)2, 1000 g, 10000 g, Ca, P, O, atomic mass of Ca, atomic mass of P, atomic mass of O, conversion factor.

since electrons are negative the answer is neagtaive