Part A. Balance the reactions:
Combustion of methane:
CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g)
Combustion of gasoline:
2 C8H18 + 25 O2 (g) → 16 CO2 (g) + 18 H2O (g)
Two common compounds used to generate energy are gasoline (C8H18) and natural gas (mostly methane (CH4). Unfortunately, both methane and gasoline produce the greenhouse gas carbon dioxide (CO2) when combusted.
a. Balance the reactions below for the combustion of methane and gasoline.
___ CH4 (g) + ___ O2 (g) → ___ CO2 (g) + ___ H2O (g)
___ C8H18 + ___ O2 (g) → ___ CO2 (g) + ___ H2O (g)
b. Which gas (25.0 g of methane or 25.0 g of gasoline) generates a larger volume of carbon dioxide at standard temperature and pressure (STP, 1 atm, 0°C) when combusted with excess oxygen? What is the volume of CO2 produced?
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