When carbon is burned in air, it reacts with oxygen to form carbon dioxide. When 16.8 gg of carbon were burned in the presence of 60.2 gg of oxygen, 15.4 gg of oxygen remained unreacted. What mass of carbon dioxide was produced?

61.6 g of CO₂ were produced

Explanation:

Let's think the combustion

C + O₂ → CO₂

First of all we determine the moles:

16.8 g . 1mol / 12 g = 1.4 moles

As the question states the oxygen is remained unreacted, the oxygen is the reactant in excess, so the limiting is the C.

1 mol of C produces 1 mol of CO₂, so 1.4 moles in the reactant will produce the same amount products.

We convert the moles to mass.

1.4 mol . 44 g / 1mol = 61.6 g

  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-

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