An Aluminum Can Has A Mass Of 15.8 Grams. How Many Aluminum Atoms Are In This Can?A. 15.8 Atoms B. 26.98 Atoms C. $2.47 \times 10^{26}$ Atoms D. $3.52 \times 10^{23}$ Atoms
Introduction
Aluminum cans are a ubiquitous part of our daily lives, used to package a wide range of products, from beverages to food. But have you ever stopped to think about the composition of these cans? What makes up the metal that surrounds the contents of our favorite drinks and snacks? In this article, we'll delve into the world of chemistry to explore the answer to this question.
The Atomic Structure of Aluminum
To understand the composition of an aluminum can, we need to start with the atomic structure of aluminum. Aluminum is a chemical element with the symbol Al and atomic number 13. It is a metal in the boron group of the periodic table and is known for its high strength-to-weight ratio, corrosion resistance, and ability to be easily molded and shaped.
The Mass of an Aluminum Can
The mass of an aluminum can is given as 15.8 grams. But what does this mean in terms of the number of aluminum atoms that make up the can? To answer this question, we need to use the concept of atomic mass.
Atomic Mass and Avogadro's Number
The atomic mass of aluminum is 26.98 grams per mole. This means that one mole of aluminum atoms has a mass of 26.98 grams. But what is a mole? A mole is a unit of measurement that represents 6.022 x 10^23 particles, whether they are atoms, molecules, or ions.
Calculating the Number of Aluminum Atoms
Now that we know the atomic mass of aluminum and the mass of the can, we can calculate the number of aluminum atoms that make up the can. We can use the following formula:
Number of atoms = (Mass of can / Atomic mass of aluminum) x Avogadro's number
Plugging in the values, we get:
Number of atoms = (15.8 g / 26.98 g/mol) x 6.022 x 10^23 atoms/mol
Solving for the Number of Atoms
Now, let's solve for the number of atoms:
Number of atoms = (15.8 g / 26.98 g/mol) x 6.022 x 10^23 atoms/mol = 0.585 x 6.022 x 10^23 atoms/mol = 3.52 x 10^23 atoms
Conclusion
In conclusion, the number of aluminum atoms in a can with a mass of 15.8 grams is approximately 3.52 x 10^23 atoms. This is a staggering number, and it highlights the incredible scale of the atomic world.
The Significance of Avogadro's Number
Avogadro's number is a fundamental constant in chemistry that represents the number of particles in one mole of a substance. It is a key concept in understanding the behavior of atoms and molecules, and it has far-reaching implications in fields such as chemistry, physics, and materials science.
The Importance of Atomic Mass
The atomic mass of an element is a critical piece of information that allows us to calculate the number of atoms in a given sample. It is a fundamental property of an element that is used to determine its chemical behavior and reactivity.
The Role of Aluminum in Our Daily Lives
Aluminum is a ubiquitous metal that plays a critical role in our daily lives. From the cans that hold our favorite beverages to the aircraft that transport us around the world, aluminum is an essential material that is used in a wide range of applications.
The Future of Aluminum
As we look to the future, it is clear that aluminum will continue to play a critical role in our daily lives. From the development of new aluminum alloys to the use of aluminum in emerging technologies such as electric vehicles and renewable energy systems, the possibilities are endless.
Conclusion
In conclusion, the number of aluminum atoms in a can with a mass of 15.8 grams is approximately 3.52 x 10^23 atoms. This is a staggering number that highlights the incredible scale of the atomic world. By understanding the atomic structure of aluminum and the concept of Avogadro's number, we can gain a deeper appreciation for the importance of this metal in our daily lives.