Question

If 4.9 moles of carbon dioxide, CO2, was produced, how many grams of water was also produced?C6H12O6 (s) + 6 O2(g) → 6 CO2 (g) + 6 H2O (g)

Answer 1

The given reaction is already balanced, that is to say, the number of atoms in the reactants matches the number of atoms in the products. In the reaction, we can see the relationship between (Carbon dioxide) CO2 and (Water) H2O. For every 6 moles of CO2 produced, 6 moles of H2O are produced, the same number of moles. This tells us that the ratio between these two products is 1 to 1.

So, if 4.9 moles of CO2 are produced we will also have 4.9 moles of H2O. Now to determine the grams of H2O we will use the mass molar of H2O equal to 18.01 g/mol and we will apply the following equation:

`\begin{gathered} \text{Mass of H}_2O=\text{ Mol of H}_2O\text{ }* Mass\text{ molar of H}_2O \\ \text{Mass of H}_2O=4.9\text{ mol}*18.01\text{ }\frac{\text{g}}{mol} \\ \text{Mass of H}_2O\text{ =88.2 g} \end{gathered}`

If 4.9 moles of carbon dioxide, CO2, was produced, 88.2 g of water was also produced.