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

a  solution  is always transparent, light passes through with no scattering from solute particles which are molecule in size. the  solution  is homogeneous and does not settle out. a colloid is intermediate between asolution  and a  suspension. while asuspension  will separate out a colloid will not.

the number of protons in the nucleus of a given element. has slight luster and conducts electricity at high temperatures like metal.but like a nonmetal,boron is brittle and does not conduct electricity well at low temperatures. in graphite, carbon is a soft,brittle solid.it is reflective,ductile,or malleable.