1. The problem statement, all variables and given/known data The complete combustion of methane is represented in the following equation: CH4(g) + 2O2 -> CO2(g) +2H2O(g) +802.5 kJ Assume that natural gas is essentially methane. The emission level of Carbon monoxide, CO(g) from the burning of natural gas is 19.14kg/MJ of energy produced. 2. Relevant equations What mass of CO(g) will be emitted when 100g of natural gas is burned? 3. The attempt at a solution I attempted to convert the 100g of methane into mol (100g/16.04g per mol) and then i multiplied the mol by it's standard molar enthalpy of formation on wikipedia (-74.9KJ/mol) to find the KJ then converted it into MJ and multiplied the methane mol with 19.14Kg/MJ. My answer was wrong. The textbook answer is 95.7 kg.