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)?

126.14 g

CH₄ (g) + 2O₂ (g) → CO₂(g) + 2H₂O(g)

We are given;

We are required to determine the mass of H₂O produced

Therefore, Moles of methane = Moles of H₂O × 2

Hence, Moles of H₂O = 7.0 moles

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

93.2 ml + 3920 ml = 4013 ml total  

(93.2 ml) * (2.03 m) / (4013 ml) = 0.0471 m

the volume in in l of the diluted solution would be 0.0471 m.