When methane (ch4) burns, it reacts with oxygen gas to produce carbon dioxide and water. the unbalanced equation for this reaction is ch4(g) + o2(g) → co2(g) + h2o(g) this type of reaction is referred to as a combustion reaction. what mass of water is produced from the complete combustion of 26.32 g of methane?

The mass of water produced is 59.22 g

Explanation:

This is the balanced equation of methane combustion:

CH₄(g) + 2O₂(g) → CO₂(g) +2H₂O(g)

This equation is balanced because we have the same amount of each element at each side of the equation:

Left side:

CH₄= 1C and 4H

2O₂ = (2x2)O = 4O

Total: 1C, 4H, and 4O

Right side:

CO₂ = 1C and 2O

2H₂O = (2x2)H + (2x1)O = 4H + 2O

Total: 1C, 4H, and 4O

Once it is balanced, we know from the equation that 1 mol of methane (1 CH₄) produces two mols of water ( 2 H₂O) when it reacts with oxygen. The mass of a mol of methane is:

Molar mass CH₄ in grams = mass of the carbon atom + mass of the four H atoms.

Molar mass CH₄ = 12 + 4 = 16 g

The same procedure with water:

Molar mass H₂O in grams = mass of the 2 H atoms + mass of the O atom

Molar mass H₂O in grams = 2 + 16 = 18 g

Hence 16 g (1 mol) CH4 will produce 36 (18 x 2)g H2O.

Therefore:

16 g CH4 ⇒ 36 g H20

26.32 g CH4 ⇒ x= 26.32 * 36 / 16 = 59.22 g.

Have a nice day!

the answer to this question is 3.

it is the most commonly accepted one