Gaseous methane CH4 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. Suppose 0.64 g of methane is mixed with 4.40 g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to 2 significant digits.

4.62g of CO₂ will be produced

Explanation:

Reaction of methane (CH₄) with oxygen (O₂) will produce carbon dioxide (CO₂) amd water (H₂O)

This reaction is also known as combustion reaction of alkanes

Equation of reaction,

CH₄ + 2O₂ → CO₂ + 2H₂O

From the equation of reaction, 1 mole of CH₄ reacts with 2 moles of O₂.

But number of moles = mass / molar mass

Molar mass of CH₄ = (12 + 4) = 16g/mol

Molar mass of O₂ = 16g/mol

Mass of CH₄ = number of moles * molar mass

Mass of CH₄ = 1 * 16 = 16g

Mass of O₂ = number of moles * molar mass

Mass of O₂ = 2 * 16 = 32g

Molar mass of CO₂ = 12 + 32 = 44g/mol

From the equation of reaction,

16g of CH₄ + 32g of O₂ produces 44g of CO₂

48g of reactants = 44g of CO₂

(0.64 + 4.4) g of reactants = y

48g of reactants = 44g of CO₂

5.04g of reactants = y g of CO₂

y = (5.04 * 44) / 48

y = 4.62g

4.62g of will be produced