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

a) the particles of the chair are strongly held together.