Calculate the amount of carbon dioxide that could be produced when
a. `1` mol of carbon is burnt in air
b. `1` moles of carbon is brunt in `16 g` of dioxygen.
`2` moles of carbon are burnt in `16 g` of dioxygen.

Explanation

The balanced chemical equation of combination of carbon in dioxygen (or air) is
`underset(1"mol")(C(s)) + underset(1"mol")(O_(2)(g)) to underset(1"mol")(CO_(2)(g))`
(i) In air, carbon will be completely burnt. 1 mol of carbon will give 1 mol of `CO_(2)` or = 44g
(ii) Since only 16 g of dioxygen is available (0.5 mol), it will combine with only 0.5 mol of carbon. Dioxygen is the limiting reagent. Thus, 0.5 mol of carbon will be burnt to give 0.5 mol of `CO_(2)` or = 22 g
(iii) In this case also, dioxygen is limiting reagent and only 0.5 mol of carbon will be burnt. It will produce 22 g of `CO_(2)`.