Liquid hexane CH3CH24CH3 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O Suppose 0.862 g of hexane is mixed with 5.1 g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Be sure your answer has the correct number of significant digits.

2.64g of CO₂ are produced

Explanation:

The reaction of hexane with O₂ is:

C₆H₁₄ + 19/2O₂ → 6CO₂ + 7H₂O

To solve this question, we must convert each mass of reactant to moles in order to find limiting reactant and, with the chemical reaction we can find the moles of carbon dioxide produced and the maximum mass produced:

Moles hexane -Molar mass: 86.18g/mol-:

0.862g * (1mol / 86.18g) = 0.01 moles

Moles Oxygen -Molar mass: 32g/mol-:

5.1g * (1mol / 32g) = 0.16 moles

For a complete reaction of 0.01 moles of hexane there are required:

0.01moles hexane * (19/2 Oxygen / 1mol Hexane) = 0.095 moles oxygen

As there are 0.16moles, limiting reactant is hexane.

0.01 moles of hexane produce:

0.01 moles * (6 moles carbon dioxide / 1 mole hexane) = 0.06 moles of CO₂.

The mass is -Molar mass CO₂: 44g/mol-:

0.06 moles of CO₂ * (44g/mol) =

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.