Mg2N2 Mass Calculation: Avogadro's Number Explained

Hey everyone! Let's dive into this 10th-grade chemistry question together and break down how to calculate the mass of a Magnesium Nitride (Mg2N2) compound that contains Avogadro's number of atoms. This might sound tricky, but don't worry, we'll go through it step-by-step. We're given the atomic masses of Magnesium (Mg) as 24 and Nitrogen (N) as 14. Understanding these concepts is super important in chemistry, so let's get started!

Understanding the Question

First, let’s make sure we understand what the question is asking. We need to find the mass (in grams) of the Mg2N2 compound. The key piece of information here is Avogadro's number, which is approximately 6.022 x 10^23. This number represents the number of atoms, molecules, or ions in one mole of a substance. So, we need to figure out how many moles of Mg2N2 contain Avogadro's number of atoms. To really nail this, we need to break down the compound and think about the atoms it contains. Understanding Avogadro's number is crucial in stoichiometry, which deals with the quantitative relationships between reactants and products in chemical reactions. This concept allows us to bridge the gap between the atomic world and the macroscopic world, making it possible to perform calculations involving measurable quantities like mass and volume. Remember, chemistry is all about understanding the relationships between different elements and compounds, and Avogadro's number is a cornerstone of these relationships. Getting this down will really help you in your chemistry journey!

Breaking Down the Compound: Mg2N2

So, let's break down this compound, Mg2N2, and see what it's made of. This compound consists of two magnesium atoms (Mg) and two nitrogen atoms (N). This is super important because we need to know the total number of atoms in one molecule of Mg2N2. In total, there are four atoms in one molecule of Mg2N2 (2 Mg atoms + 2 N atoms). Now, why is this important? Because the question specifies "Avogadro's number of atoms." We need to relate the number of atoms in one molecule to Avogadro's number to find out how many moles of the compound we have. Think of it like this: we're trying to find a connection between the microscopic world of atoms and the macroscopic world of grams that we can measure in the lab. Breaking down the compound formula is the first step in making that connection. This process highlights the importance of understanding chemical formulas and their significance in determining the composition of a compound. Remember, the subscripts in a chemical formula tell us the number of atoms of each element present in one molecule of the compound. Misinterpreting these subscripts can lead to incorrect calculations, so pay close attention to them! Grasping the composition of Mg2N2 in terms of its constituent atoms is the cornerstone for solving the problem, allowing us to proceed towards calculating the mass. Now that we've got this down, let's move on to the next step.

Relating Atoms to Moles

Okay, so we know that one molecule of Mg2N2 has 4 atoms. Now we need to figure out how many moles of Mg2N2 contain Avogadro's number (6.022 x 10^23) of atoms. Since 1 mole contains 6.022 x 10^23 entities (in this case, atoms), we need to consider that each molecule of Mg2N2 contains 4 atoms. Think of it like this: if you want a dozen apples (12 apples), and each bag has 4 apples, you only need 3 bags (12 apples / 4 apples per bag = 3 bags). Similarly, we need to figure out how many “bags” (moles of Mg2N2) we need to get Avogadro's number of atoms. To do this, we divide Avogadro's number by the number of atoms per molecule: (6.022 x 10^23 atoms) / (4 atoms/molecule) = 1.5055 x 10^23 molecules. Now we need to convert this number of molecules into moles. To do that, we divide by Avogadro's number again! (1.5055 x 10^23 molecules) / (6.022 x 10^23 molecules/mol) = 0.25 moles. So, we have 0.25 moles of Mg2N2. This step is crucial because it bridges the gap between the number of atoms and the amount of substance in moles, which is essential for calculating the mass. Make sure you understand this conversion process thoroughly. Getting a handle on the relationship between atoms, molecules, and moles is a fundamental concept in chemistry. Now that we know how many moles of Mg2N2 we're dealing with, we're just one step away from finding the mass!

Calculating the Molar Mass of Mg2N2

Alright, we're on the home stretch! To find the mass, we need to calculate the molar mass of Mg2N2. Remember, the molar mass is the mass of one mole of a substance, and it's calculated by adding up the atomic masses of all the atoms in the compound. We know the atomic mass of Magnesium (Mg) is 24 and the atomic mass of Nitrogen (N) is 14. In one molecule of Mg2N2, we have 2 Mg atoms and 2 N atoms. So, the molar mass calculation looks like this: (2 Mg atoms * 24 g/mol) + (2 N atoms * 14 g/mol) = 48 g/mol + 28 g/mol = 76 g/mol. This means one mole of Mg2N2 weighs 76 grams. Calculating the molar mass is a fundamental skill in chemistry, and it's essential for converting between moles and grams. Always double-check your calculations and make sure you're using the correct atomic masses from the periodic table. Understanding molar mass is critical for quantitative analysis in chemistry, allowing us to predict the amounts of reactants and products involved in chemical reactions. Now that we have the molar mass, we can finally calculate the mass of the compound in the question.

Final Calculation: Mass of Mg2N2

Okay, guys, we've got all the pieces of the puzzle! We know we have 0.25 moles of Mg2N2, and we know the molar mass of Mg2N2 is 76 g/mol. To find the mass, we simply multiply the number of moles by the molar mass: Mass = (number of moles) * (molar mass) Mass = 0.25 moles * 76 g/mol Mass = 19 grams. So, the mass of Mg2N2 compound that contains Avogadro's number of atoms is 19 grams. Awesome! We did it! This final calculation ties everything together, demonstrating the practical application of the concepts we've discussed. Remember, always include the units in your calculations to ensure that your answer is in the correct units. This step reinforces the importance of using molar mass as a conversion factor between moles and mass, a key concept in stoichiometry. Now you’ve seen how to approach this type of problem, breaking it down into smaller, manageable steps. Practice makes perfect, so try similar problems to solidify your understanding.

Conclusion

So, to recap, the mass of the Mg2N2 compound containing Avogadro's number of atoms is 19 grams. We found this by first understanding the question and identifying that we needed to work with Avogadro's number. Then, we broke down the compound to see how many atoms were in each molecule. We related the number of atoms to moles, calculated the molar mass, and finally, calculated the mass. Remember, chemistry problems often seem complex at first, but breaking them down into smaller steps makes them much easier to solve. Keep practicing, and you'll become a chemistry whiz in no time! Understanding these concepts builds a strong foundation for further studies in chemistry, allowing you to tackle more complex problems with confidence. Don't be afraid to ask questions and seek help when you need it. Chemistry can be challenging, but it's also incredibly fascinating! Keep up the great work, and you'll ace your 10th-grade chemistry class! Remember that consistent effort and a clear understanding of the underlying principles are the keys to success in chemistry. Good luck with your studies!