The balanced chemical equation for the combustion of methane is:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
Now, let’s analyze the statement: ‘One gram of CH4 reacts with two grams of O2 producing one gram of C.’
This statement is incorrect. During combustion, methane (CH4) reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). There is no elemental carbon (C) produced in this reaction; instead, all the carbon in methane is converted to carbon dioxide. Therefore, the accurate interpretation of this reaction focuses on the production of CO2 and H2O, and not on any free carbon.
In terms of stoichiometry, if you burn one mole of CH4 (which weighs about 16 grams), you need two moles of O2 (about 32 grams) to produce one mole of CO2 (about 44 grams) and two moles of H2O (about 36 grams). Hence, the masses do not correspond to the statement as given.
In conclusion, the combustion of methane results in the production of carbon dioxide and water, and the statement about producing elemental carbon is false.