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.

Question

When methane, CH4, is combusted, it produces carbon dioxide, CO2, according to the unbalanced equation: CH4 + O2 → CO2 + H2O.

1 mol of methane is 16 grams that produces 6.25 moles of  CO2

when it is burnt

Explanation:

1 mol of methane is 16 grams. Therefore, if you have 100 grams of methane, it means that you have  100/16=6.25moles of methane.

When you burn 6.25 moles of methane, you produce 6.25 moles of carbondioxide.

Your reaction is wrong though. I want to correct it.

CH4+2O2→CO2+2H2O

When you burn 6.25 moles of methane, you need 12.5 moles of oxygen gas.

When you burn 6.25 moles of methane, you produce 6.25 moles of carbondioxide (275 grams of  CO2) and 12.5 moles of water vapour (225 grams of  H2O).

Hope this helps!