Heating 2.40 g of the oxide of metal x (molar mass of x = 55.9 g/mol) in carbon monoxide (co) yields the pure metal and carbon dioxide. the mass of the metal product is 1.68 g. from the data given, show that the simplest formula of the oxide is x2o3 and write a balanced equation for the reaction.

The molecular formula of the oxide of metal be . The balanced equation for the reaction is given by:

Explanation:

Let the molecular formula of the oxide of metal be

Mass of metal product = 1.68 g

Moles of metal X =

1 mol of metal oxide produces 2 moles of metal X.

Then 0.03005 moles of metal X will be produced by:

of metal oxide

Mass of 0.01502 mol of metal oxide = 2.40 g (given)

y = 2.999 ≈ 3

The molecular formula of the oxide of metal be . The balanced equation for the reaction is given by:

solute : a solute is a substance that is dissolved in another substance is known as a solvent. it is mixed with a special mixture know as homogeneous mixture.

solvent: a solvent is a substance that dissolved a solute, which results in a solution is known as solvent.

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-