For the complete combustion of 0.477 g CO, it must be converted to CO2.
2 CO(g) + O2(g) → 2 CO2(g)
When hydrocarbons are burned in a limited amount of air, both CO and CO2 form. When 0.460 g of a particular hydrocarbon was burned in air, 0.477 g of CO, 0.749 g of CO2, and 0.460 g of H2O were formed.
How many grams would have been required for complete combustion?
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