# 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;

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