If a car produces 62g of co2, how many grams of o2 are used up in the reaction?

Given:

Amount of CO2 produced = 62 g

To determine:

Amount of O2 consumed

Explanation:

If ethanol (C2H5OH) is the fuel used during combustion then the reaction is:

C2H5OH + 3O2 → 2CO2 + 3H2O

Based on the reaction stoichiometry:

3 moles of O2 will produce 2 moles of CO2

# moles of CO2 produced = 62 g/ 44 g.mol-1 = 1.4091 moles

Therefore,

# moles of O2 consumed = 1.4091 *3/2 = 2.1137 moles

Mass of O2 used up = 2.1137 moles * 32 g/mole = 67.64 g

Ans: The mass of O2 used up during combustion of ethanol would be around 68 g

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.  

1.43 x 10^-11 j the guy commented the awnser just making sure u see it .