How many moles of calcium oxide will be produced when 1.6 moles of iron(iii)oxide reacts with calcium phosphate according to the following (unbalanced) reaction: fe2o3 + ca3(po4)2 —> fe(po4) + cao

4.8 mol

Step-by-step explanation:

The balanced equation is

Fe₂O₃ + Ca₃(PO₄)₂ ⟶2FePO₄ + 3CaO

You want to convert moles of Fe₂O₃ to moles of CaO.

The molar ratio is 3 mol CaO:1 mol Fe₂O₃.

Moles of CaO = 1.6 mol Fe₂O₃ × (3 mol CaO/1 mol Fe₂O₃)

Moles of CaO = 4.8 mol CaO

The reaction will produce 4.8 mol of CaO.

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.