What mass of water is produced from the complete combustion of 7.10*10-3 g of methane? Express your answer with the appropriate units.

16 mg of water can be produced by 7.1*10⁻³ g of CH₄

Explanation:

This is the reaction:

CH₄ + 2O₂ → CO₂ + 2H₂O

In a combustion, oxgen is a reactant with another compound, and the products are always water and carbon dioxide

1 mol of methane can produce 2 moles of water. Ratio is 1:2

If we convert the mass to moles → 7.1*10⁻³ g. 1 mol / 16g = 4.43*10⁻⁴ mol

In this reaction I would produce the double of moles I have from methane, so If I have 4.43*10⁻⁴ moles of methane I would produce 8.87*10⁻⁴ moles of water.

What mass of water, corresponds to 8.87*10⁻⁴ moles?

8.87*10⁻⁴ mol. 18g / 1mol = 0.016 g which is actually the same as 16 mg