$4 Al (s) + 3 O_2(g) \rightarrow 2 Al_2 O_3(s)$

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rylee67789 rylee67789

03-11-2026
Chemistry

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$4 Al (s) + 3 O_2(g) \rightarrow 2 Al_2 O_3(s)$

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GinnyAnswer GinnyAnswer · Answer 1 · 2026-11-03T12:07:51-05:00

Identify the synthesis reaction where aluminum reacts with oxygen gas to form aluminum oxide.
Interpret the stoichiometric coefficients: 4 moles of Al react with 3 moles of O2 to yield 2 moles of Al2O3.
Verify the balance of atoms: there are 4 aluminum atoms and 6 oxygen atoms on both sides of the equation, ensuring conservation of mass.
Note the physical states: aluminum and aluminum oxide are solids, while oxygen is a gas.

Explanation

Analysis of the Chemical Equation

The chemical equation $4 \text{Al} (s) + 3 \text{O}_2 (g) \rightarrow 2 \text{Al}_2 \text{O}_3 (s)$ represents a synthesis reaction, also known as a combination reaction. In this reaction, aluminum metal (Al) reacts with oxygen gas (O2) to form aluminum oxide (Al2O3), which is a common protective oxide layer that forms on aluminum surfaces. The letters in parentheses indicate the physical states of the substances: $(s)$ stands for solid, and $(g)$ stands for gas.

Interpreting Stoichiometric Coefficients

The stoichiometric coefficients in the equation tell us the molar ratios required for the reaction to proceed. Specifically, the coefficient $4$ in front of Al, $3$ in front of O2, and $2$ in front of Al2O3 indicates that for every $4$ moles of aluminum consumed, $3$ moles of oxygen gas are required, which results in the formation of $2$ moles of aluminum oxide. This ratio is fundamental to understanding the stoichiometry of the reaction, ensuring that the reactants are consumed in precise proportions.

Conservation of Mass Verification

To verify that the law of conservation of mass is satisfied, we must confirm that the number of atoms of each element is the same on both sides of the equation.
For Aluminum (Al):

Left side: $4$ atoms of Al.
Right side: $2 \times 2 = 4$ atoms of Al.

For Oxygen (O):

Left side: $3 \times 2 = 6$ atoms of O.
Right side: $2 \times 3 = 6$ atoms of O.

Since the number of atoms for both aluminum and oxygen are equal on both sides, the equation is balanced, meaning mass is conserved.

Final Conclusion

In summary, the equation $4 \text{Al} (s) + 3 \text{O}_2 (g) \rightarrow 2 \text{Al}_2 \text{O}_3 (s)$ is a balanced chemical expression where:

The reactants are $4$ moles of solid aluminum and $3$ moles of gaseous oxygen.
The product is $2$ moles of solid aluminum oxide.

This balance ensures that matter is neither created nor destroyed, adhering to the fundamental principles of chemical science. The final interpretation is that this reaction demonstrates the oxidation of aluminum.

Examples

In everyday life, this chemical reaction is crucial for the durability of aluminum products. When aluminum is exposed to the atmosphere, it quickly reacts with oxygen to form a thin, durable layer of aluminum oxide (Al2O3) on its surface. This process, called passivation, prevents further oxidation and corrosion of the underlying metal, which is why aluminum window frames, soda cans, and aerospace components can last for years outdoors without rusting like iron. Understanding this stoichiometry helps engineers determine the thickness of the oxide layer needed for various industrial applications.