20 POINTS When methane, CH4, is combusted, and 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 in and emit 27 grams of carbon dioxide. Discuss whether or not this reaction obeys the law of conservation of mass.

Balanced equation: CH4 + 2O2=CO2 + 2H2O

It is possible for 10g of methane to produce 27 g of CO2 because for every mole of ch4 there is about 16 g and for every mole of ch4 there is 1 mole co2 and for every mole co2 there is 44g of co2. (it makes more sense mathematically as shown in the explanation.) Since we can convert 10 g of CH4 into 27 grams of CO2 without losing or adding extra mass, law of conservation of mass is obeyed.

Explanation:

we know that CH4 +02 —>CO2 + H2O

On the left we have 4 hydrogen atoms, 2 oxygen and one carbon.

On the right, we have 2 hydrogen, 3 oxygen, and one carbon.

We start by multiplying water by 2 so that both sides have 4 hydrogen.

CH4 +02 —>CO2 + 2H2O

On the left we have 4 hydrogen atoms, 2 oxygen and one carbon.

On the right, we have 4 hydrogen, 4 oxygen, and one carbon.

We finish balancing by multiplying the oxygen on the left by 2 so both sides have 4 oxygen

CH4 +202 —>CO2 + 2H2O

We can prove that 10g of ch4 produces 27g of co2 by using stoichiometry:

they are all solids.