Question

How many grams are in $2.3 \times {10^4}$ mol of calcium phosphate, $C{a_3}{(P{O_4})_2}$?

Answer 1

Hint: The mass of the compound where the number of moles is given is calculated by multiplying the number of moles with the molecular weight. The molecular weight can be calculated using the atomic weight of the atom given in the periodic table.

Complete step by step answer:
It is given that the moles present in calcium phosphate is $2.3 \times {10^4}$moles.
The mass of the substance is defined as the measure of the amount of matter present in the substance. The mass is measured in grams. The mole of any substance is equal to the value of $6.022 \times {10^{23}}$number be its atom or any molecule.
The formula relating the mass and moles shows that the moles is calculated by dividing the mass of the substance with the molecular weight.
The molecular weight is calculated by summing up the atomic weight of each atom present in the compound and if the atoms are present in number so the number is multiplied by the atomic weight.
The chemical formula of calcium phosphate is $C{a_3}{(P{O_4})_2}$.
The atomic weight of calcium is 40.1.
The atomic weight of phosphorous is 31.
The atomic weight of oxygen is 16.
$ \Rightarrow Molecular\;weight = 40.1 \times 3 + 31 \times 2 + 16 \times 3$
$ \Rightarrow Molecular\;weight = 310.3g$
The formula is shown below.
$n = \dfrac{m}{M}$
Where,
n is the number of moles
m is the mass
M is the molecular weight
To calculate the mass, substitute the values in the above equation.
$ \Rightarrow 2.3 \times {10^4} = \dfrac{m}{{310.3g/mol}}$
$ \Rightarrow m = 7136900g$
Therefore, 7136900 grams are in $2.3 \times {10^4}$ moles of calcium phosphate.

Note:
The atomic weight is the average sum of the masses of each isotope of the atom where each isotope is multiplied with the natural abundance value.