Butane gas (C4H10) is used as the fuel in disposable lighters. It burns in oxygen to form carbon dioxide gas and water vapor. What mass of carbon dioxide is produced when 4.65 g of butane is burned in 10.0 g of oxygen? How many grams of the excess reactant remain unreacted when the reaction is over? The balanced equation is: 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g)
Butane gas (C4H10) is used as the fuel in disposable lighters. It burns in oxygen to form carbon dioxide gas
and water vapor. What mass of carbon dioxide is produced when 4.65 g of butane is burned in 10.0 g of
oxygen? How many grams of the excess reactant remain unreacted when the reaction is over?
The balanced equation is: 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g)
a) 4.65 g of CO2 is produced and 5.35 g of excess oxygen remains
b) 14.1 g of CO2 is produced and 5.35 g of excess butane remains
c) 8.46 g of CO2 is produced and 2.79 g of excess oxygen remains
d) 8.46 g of CO2 is produced and 1.86 g of excess butane remains
e) 2.79 g of CO2 is produced and 5.35 g of excess oxygen remains
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