What mass of carbon dioxide is formed by the complete combustion of 885g of methanol?

2CH3OH + 3O2 ==> 2CO2 + 4H2O

mols methanol = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols methanol to mols CO2.
The convert mols CO2 to grams. g = mols x molar mass.

To calculate the mass of carbon dioxide formed by the complete combustion of methanol, we need to use the balanced chemical equation for the combustion reaction. The balanced equation for the combustion of methanol (CH3OH) produces carbon dioxide (CO2) and water (H2O):

2CH3OH + 3O2 -> 2CO2 + 4H2O

From the equation, we can see that 2 moles of methanol react to form 2 moles of carbon dioxide.

To find the number of moles of methanol in 885g, we need to use the molar mass of methanol (32.04 g/mol).

Moles of methanol = mass of methanol / molar mass of methanol

Moles of methanol = 885g / 32.04 g/mol ≈ 27.59 mol

Since the stoichiometry of the reaction is 2 moles of methanol to 2 moles of carbon dioxide, we can conclude that 27.59 moles of methanol will produce 27.59 moles of carbon dioxide.

Now, to find the mass of carbon dioxide formed, we multiply the number of moles of carbon dioxide by its molar mass (44.01 g/mol).

Mass of carbon dioxide = moles of carbon dioxide × molar mass of carbon dioxide

Mass of carbon dioxide = 27.59 mol × 44.01 g/mol ≈ 1213 g

Therefore, the mass of carbon dioxide formed by the complete combustion of 885g of methanol is approximately 1213 grams.