When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide.

C(s) + O2(g)--> CO2(g)

However, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result.

2 C(s) + O2(g)--> 2 CO(g)

What mass of each product is expected when a 4.50 g sample of pure carbon is burned under each of these conditions?