How much air is needed to burn 12 g of butane?
The butane oxidation reaction is described by the following chemical reaction equation.
2C4H10 + 13O2 = 8CO2 + 10H2O;
According to the coefficients of this equation, 13 oxygen molecules are required to oxidize 2 butane molecules. In this case, 8 molecules of carbon dioxide are synthesized.
Let’s calculate the amount of butane available.
To do this, divide the weight of the available gas by the weight of 1 mole of this gas.
M C4H10 = 12 x 4 + 10 = 58 grams / mol;
N C4H10 = 12/58 = 0.207 mol;
The amount of oxygen will be.
N O2 = 0.207 x 13/2 = 1.346 mol;
Let’s calculate the gas volume. To do this, multiply the amount of substance by the volume of 1 mole of gas.
Its volume will be: V O2 = 1.346 x 22.4 = 30.15 liters;
The oxygen content in the air is 21%.
The required air volume will be:
V air = 30.15 / 0.21 = 143.571 liters;