When methane, ch4, is combusted, it produces carbon dioxide, co2, according to the unbalanced equation: ch4 + o2 → co2 + h2o. write the balanced equation for this reaction, and explain how it is possible for 10 grams of methane fuel to burn and emit 27 grams of carbon dioxide. discuss whether or not this reaction obeys the law of conservation of mass.

Answer : The balanced equation for this reaction is,

Solution : Given,

Molar mass of = 16 g/mole

Molar mass of = 44 g/mole

Moles of =

Moles of = 0.625 moles

From the balanced equation we conclude that

1 mole of gives 1 mole of

0.625 moles of gives of

Moles of = 0.625 moles

Now we have to calculate the Mass of .

Mass of = Moles of × Molar mass of = 0.625 moles × 44 g/mole = 27.5 g

Mass of = 27.5 g

It is possible for 10 grams of methane fuel to burn and emit 27 grams of carbon dioxide.

For Net balanced chemical equation:

The mass of reactant side,

The mass of product side,

That means, the mass of product is equal to the mass of reactant. The mass remains conserved.

For Unbalanced chemical equation:

The mass of reactant side,

The mass of product side,

This means, the mass of product is not equal to the mass of reactant. The mass is not conserved.

The Net balanced chemical equation obeys the law of conservation of mass but unbalanced equation are not obeys the law of conservation of mass.

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