# According to the following reaction how many moles of carbon dioxide will be formed upon the complete reaction of 28.2 grams of carbon (graphite) with excess oxygen gas?

## carbon (graphite) (s) + oxygen (g) $\to$ carbon dioxide (g)

Nov 3, 2016

Each mole of carbon gives $44 \cdot g$ of carbon dioxide gas upon oxidation.

#### Explanation:

$C \left(s\right) + {O}_{2} \left(g\right) \rightarrow C {O}_{2} \left(g\right)$.

The $1 : 1$ stoichiometry is clear: moles of carbon, and dioxygen gas are equivalent to the moles of carbon dioxide gas generated.

We start with $\frac{28.2 \cdot g}{12.01 \cdot g \cdot m o l} = 2.35 \cdot m o l$ $C$, and thus $2.35 \cdot m o l \times 44.01 \cdot g \cdot m o {l}^{-} 1$ $C {O}_{2} \left(g\right)$ are evolved.

Suppose that less than $100 \cdot g$ of gas were collected in the experiment. Barring error on the part of the experimenter, what would be a reasonable explanation?