Question

How many moles of magnesium phosphate $[M{g_3}{(P{O_3})_2}]$ will contain $0.25$ moles of oxygen atoms?

Answer 1

Hint: In the above given question we need to look at how many moles of oxygen atom constitute one mole of magnesium phosphate and then by comparing their ratio, calculate the amount of magnesium phosphate in $0.25$ moles of oxygen atoms.

Complete answer:
Now in the above question we have been asked how much of magnesium phosphate will contain $0.25$ moles of oxygen atoms.
Now to calculate that first we need to calculate the number of moles of oxygen in one mole of magnesium phosphate.
On observing the formula of magnesium phosphate that is $[M{g_3}{(P{O_3})_2}]$ we can say that in one mole of magnesium phosphate of there are about six moles of oxygen atoms.
We calculate that by opening up the formula and observing their base coefficient and we see that one mole of magnesium phosphate has three moles of magnesium atom and 2 moles of phosphate. Now one mole of phosphate contains about three moles of oxygen atoms, then two moles of phosphate would contain twice the number of that, i.e., six moles of oxygen atoms.
Now in the question we are given that we have about $0.25$ moles of oxygen and need to calculate the moles of magnesium phosphate, we have six moles of oxygen atoms in one mole of magnesium phosphate then $0.25$ moles would have let's say $x$ moles of magnesium phosphate , the ratio of oxygen to magnesium phosphate need to remain constant
$\dfrac{1}{6} = \dfrac{x}{{0.25}}$
$x = 0.04$
$0.25$ moles of oxygen atoms are there in $0.04$ moles of magnesium phosphate.

Note:
Magnesium phosphate is widely used in medication in order to support the relaxation of muscles. This compound is also used to prevent the cramping of muscles. Magnesium phosphate is also used to prevent vitamin E deficiency.