Natural gas is primarily methane, CH4, and is used to heat homes. A typical home is approximately 2000 ft2 and the ceilings are 8 ft high. The following data may be helpful: The heat capacity of air is 1.01 J/g·K and the and the enthalpy of combustion of methane is -890.8 kJ/mol. Assume that the molecular weight of air is the same as nitrogen, its major component.
How many grams of methane are required to raise the temperature in the home from 40.°F to 69°F?
How many grams of CO2 does this reaction produce?
For the first part, i have: Calculated the volume of the house. Calculated the density of air and therefore mass of air.
energy to raise the house's temperature = mass of air * specific heat * temperature change
Divided the energy required by the heat of combustion for methane, that gives you moles of methane needed. mass of methane = moles of methane * 16.044 g/mole.
Which i ended up getting 4689.46g but it is wrong, Any help?