Question

Enter your answer in the provided box. The balanced equation for the combustion of ethanol (ethyl alcohol) is: C2H5OH() + 3O2(g) → 2CO2(g) + 3H2O(g) How many g of CO2 will be produced by the combustion of 4 mol of ethanol? g CO2

Answer 1

Answer: The mass of carbon dioxide produced is 352 grams

Explanation:

We are given:

Moles of ethanol = 4 mol

For the given chemical equation:

$C_2H_5OH(g)+3O_2(g)\rightarrow 2CO_2(g)+3H_2O(g)$

By Stoichiometry of the reaction:

1 mole of ethanol produces 2 moles of carbon dioxide

So, 4 moles of ethanol will produce = $\frac{2}{1}\times 4=8mol$ of carbon dioxide

To calculate the mass of carbon dioxide, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Moles of carbon dioxide = 8 moles

Molar mass of carbon dioxide = 44 g/mol

Putting values in above equation:

$8mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(8mol\times 44g/mol)=352g$

Hence, the mass of carbon dioxide produced is 352 grams