Question

Write a balanced chemical equation between magnesium chloride and sodium phosphate. Determine the grams of magnesium chloride that are needed to produce 1.33 x 10^{23} formula units of magnesium phosphate.

Answer 1

The grams of MgCl₂ that are needed are 63.1 g

Step-by-step explanation:

First of all, try to think the equation and ballance it. This is it:

3MgCl₂ + 2Na₃PO₄ → Mg₃(PO₄)₂ + 6NaCl

Let's convert our f.u in mol

1 mol = 6.02x10²³ formula units (Avogadro's number)

So f.u / Avogadro = mol

1.33x10²³ / 6.02x10²³ = 0.221 moles.

So 1 mol of phosphate sodium comes from 3 mol of magnesium chloride.

How many mol of magnesium chloride are necessary, for 0.221 mol of phosphate.?

0.221 moles .3 = 0.663 moles.

Molar mass of MgCl₂ is 95.2 g/m

0.663 moles . 95.2 g/m = 63.1 g