Question

CH, (g) + 20 (g) → CO(g) + 2H 0(g)
Determine the mass of H,0 (9) produced in the complete combustion of 3.5 moles of methane (CH)?

Answer 1

Answer:

126.14 g

Explanation:

• Complete combustion of hydrocarbons yields water and carbon dioxide.
• Methane is a hydrocarbon in the homologous series known as alkanes.
• Methane undergoes combustion in air to produce water and carbon dioxide according to the equation below.

CH₄ (g) + 2O₂ (g) → CO₂(g) + 2H₂O(g)

We are given;

• 3.5 moles of Methane

We are required to determine the mass of H₂O produced

Step 1: Moles of H₂O produced

• From the equation 1 mole of methane undergoes combustion to produce 2 mole of H₂O.

Therefore, Moles of methane = Moles of H₂O × 2

Hence, Moles of H₂O = 7.0 moles

Step 2: Mass of H₂O produced

We know that; mass = Moles × Molar mass

Molar mass of water = 18.02 g/mol

Therefore;

Mass of water = 7.0 moles × 18.02 g/mol

                       = 126.14 g

Thus, the mass of water produced is 126.14 g