Balance the following chemical equation: C2H60+02 → CO2 + H20
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Answer:
391.28771 pounds of carbon-dioxide was released into the atmosphere when 22.0 gallon tank of gasoline is burned in an automobile engine.
Explanation:
Density of the gasoline ,d= 0.692 g/mL
Volume of gasoline in an tanks,V = 22.0 gallons = 83,279.02 mL
Let mass of the gasoline be M
M = V × d = 83,279.02 mL × 0.692 g/mL=57,629.081 g
Given that gasoline is primarily octane.
Mass of octane burnt in the tank = M = 57,629.081 g
Moles of octane =
According to reaction, 2 moles of octane gives 16 moles of carbon-dioxide.
Then 505.1637 mol of octane will give:
of carbon-dioxide
Mass of 4,041.3100 mol of carbon-dioxide:
4,041.3100 mol × 44.01 g/mol = 177,858.05 g
Mass of carbon-dioxide produced in pounds = 391.28771 pounds
391.28771 pounds of carbon-dioxide was released into the atmosphere when 22.0 gallon tank of gasoline is burned in an automobile engine.