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When methane, CH4, is combusted, it produces carbon dioxide, CO₂, according to the unbalanced equation: CH4 +0₂ - 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. (5 points)

Sagot :

Oseniidn

The balanced equation will be [tex]CH_4 + 2O_2 --- > CO_2 + 2H_2O[/tex]

Stoichiometric problems

The balanced equation of the reaction would be as follows:

[tex]CH_4 + 2O_2 --- > CO_2 + 2H_2O[/tex]

The mole ratio of methane to carbon dioxide is 1:1.

10 grams of methane will give 10/16 = 0.625 moles

0.625 moles of carbon dioxide would give 0.625 x 44.01 = 27.506 grams.

Thus, 10 grams of methane will produce approximately 27 grams of carbon dioxide stoichiometrically.

The reaction obeys the law of conservation of mass because the atoms of all the elements before and after the reaction are balanced.

More on stoichiometric problems can be found here: https://brainly.com/question/14465605

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