Burning of methane is a
combustion reaction. CH₄(g) reacts with O₂(g) and gives CO₂(g) and H₂O(l) as the products.
The balance reaction equation is
CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l)
Moles (mol) = mass (g) / molar mass (g/mol)
Mass of CH₄ =
13.15 g
Molar mass of CH₄ = 16.04 g/mol
Moles of CH₄ = 13.15 g /16.04 g/mol
= 0.82 mol
The stoichiometric ratio between
CH₄ and
H₂O is
1 : 2.Hence,
moles of H₂O formed = moles of reacted CH₄ x 2
= 0.82 x 2
= 1.64 mol
According to the Avogadro's constant, 1 mole of substance
has 6.022 × 10²³ particles.
Hence,
number of H₂O molecules formed = 1.64 mol x 6.022 ×
10²³ mol
= 9.88 x 10²³
Hence, answer is 9.88 x 10²³ of molecules.
