# Hm many grams of CO_2 would be formed from 30 grams of C_7H_8 in the following reaction C_7H_8 + O_2 -> CO_2 + H_2O?

Jan 29, 2016

Approx. $100$ $g$.

#### Explanation:

A balanced equation representing the complete combustion of toluene is absolutely necessary:

${C}_{7} {H}_{8} + 9 {O}_{2} \rightarrow 7 C {O}_{2} + 4 {H}_{2} O$

This tells us that for every mole of toluene, 7 moles carbon dioxide gas are evolved under conditions of complete combustion. So we need to find (i) molar quantity of toluene, and (ii) equivalent molar quantity of carbon dioxide.

Moles of ${C}_{7} {H}_{8}$ $=$ $\frac{30 \cdot \cancel{g}}{92.14 \cdot \cancel{g} \cdot m o {l}^{-} 1}$ $=$ $0.326$ $\text{mol}$

Given the stoichiometry of the rxn, 7 mol carbon dioxide are produced from 1 mol toluene. Thus, the answer is:

$7$ $\times$ $44.0$ $g \cdot \cancel{m o {l}^{-} 1}$ $\times 0.326$ $\cancel{m o l}$ $=$ ??g

If $1$ '$m o l$ of gas occupies $25.4$ ${\mathrm{dm}}^{3}$ under standard conditions, what is the volume of this molar quantity of $C {O}_{2}$?