# How many grams of CO_2 and grams of H_2O are produced when 52.0 g C_2H_2 burns in oxygen?

May 20, 2016

$H - C \equiv C - H \left(g\right) + \frac{5}{2} {O}_{2} \left(g\right) \rightarrow 2 C {O}_{2} \left(g\right) + {H}_{2} O$
$H - C \equiv C - H \left(g\right) + \frac{5}{2} {O}_{2} \left(g\right) \rightarrow 2 C {O}_{2} \left(g\right) + {H}_{2} O \left(l\right)$
$\text{Moles of acetylene}$ $=$ $\frac{52.0 \cdot g}{26.04 \cdot g \cdot m o {l}^{-} 1}$ $=$ $2 \cdot m o l$
Given the molar equivalence, $4 \cdot m o l \times 44.0 \cdot g \cdot m o {l}^{-} 1$ $C {O}_{2}$ are produced, as well as $36.0 \cdot g$ water.