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

The mass of carbon dioxide produced is 352 grams

Explanation:

We are given:

Moles of ethanol = 4 mol

For the given chemical equation:

By Stoichiometry of the reaction:

1 mole of ethanol produces 2 moles of carbon dioxide

So, 4 moles of ethanol will produce = of carbon dioxide

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

Moles of carbon dioxide = 8 moles

Molar mass of carbon dioxide = 44 g/mol

Putting values in above equation:

Hence, the mass of carbon dioxide produced is 352 grams

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.