Silver Sulfide Formation: Calculate Mass From 0.6 Mol Silver

Hey guys! Today, we're diving into a fascinating chemistry problem: calculating the mass of silver sulfide formed when silver reacts with sulfur. This is a classic example of a stoichiometry problem, and it's super important to understand the underlying principles. We'll break it down step by step, so you can confidently tackle similar problems in the future. So, let's get started and unravel this chemical equation together!

Understanding the Reaction

Before we jump into the calculations, let's first grasp the core concept of this reaction. Silver sulfide (Ag₂S), the black tarnish you often see on silverware, is created when silver (Ag) reacts with sulfur (S). This is a classic chemical reaction, and understanding it is crucial for solving our problem. The reaction essentially involves the combination of silver and sulfur atoms to form a new compound, silver sulfide. The black color of silver sulfide is a distinctive characteristic and a telltale sign of this reaction. Think about it – when your favorite silver jewelry loses its shine and turns black, it's likely due to this very reaction occurring with sulfur compounds in the air!

To fully understand this reaction, we need to consider the balanced chemical equation. This equation tells us the exact ratio in which silver and sulfur react. The balanced equation is: 2 Ag + S → Ag₂S. This equation is the foundation for all our calculations, providing us with the molar ratios needed to determine the mass of silver sulfide formed. Always remember, guys, balancing chemical equations is a fundamental skill in chemistry, and it's essential for accurate stoichiometric calculations. Without a balanced equation, our calculations would be like trying to build a house without a blueprint – a recipe for disaster! So, make sure you're comfortable with balancing equations before moving on to the next step.

Key Concepts

• Reactants and Products: In this reaction, silver (Ag) and sulfur (S) are the reactants, while silver sulfide (Ag₂S) is the product.
• Balanced Equation: The balanced chemical equation (2 Ag + S → Ag₂S) is essential for determining the molar ratios between the reactants and the product.
• Molar Ratio: The balanced equation tells us that 2 moles of silver react with 1 mole of sulfur to produce 1 mole of silver sulfide. This is the crucial piece of information we'll use for our calculations. Think of the molar ratio as the recipe for this chemical reaction – it tells us exactly how much of each ingredient (reactants) we need to get the desired outcome (product).

Calculating Moles of Silver Sulfide

Now, let's get down to the nitty-gritty of the calculation. We are given that we have 0.6 moles of silver (Ag) reacting. Our goal is to figure out how many moles of silver sulfide (Ag₂S) will be formed from this amount of silver. This is where the molar ratio from the balanced equation comes into play. Remember, the balanced equation (2 Ag + S → Ag₂S) tells us that 2 moles of silver produce 1 mole of silver sulfide. This is our conversion factor, the magical key that unlocks the solution to our problem!

To find the moles of silver sulfide, we use the following proportion:

(Moles of Ag₂S) / (Moles of Ag) = (1 mole Ag₂S) / (2 moles Ag)

We know the moles of silver (0.6 moles), so we can plug that into the equation:

(Moles of Ag₂S) / (0.6 moles Ag) = (1 mole Ag₂S) / (2 moles Ag)

Now, we can solve for the moles of Ag₂S by multiplying both sides of the equation by 0.6 moles Ag:

Moles of Ag₂S = (0.6 moles Ag) * (1 mole Ag₂S) / (2 moles Ag)

Moles of Ag₂S = 0.3 moles

So, we've figured out that 0.6 moles of silver will produce 0.3 moles of silver sulfide. See how the molar ratio acted as a bridge, allowing us to convert from moles of one substance (silver) to moles of another (silver sulfide)? This is the power of stoichiometry, guys!

Key Steps

• Identify the Given Information: We started with 0.6 moles of silver.
• Use the Molar Ratio: We used the ratio from the balanced equation (2 moles Ag : 1 mole Ag₂S) to relate the moles of silver to the moles of silver sulfide.
• Calculate Moles of Product: We calculated that 0.6 moles of silver will produce 0.3 moles of silver sulfide.

Determining the Molar Mass of Silver Sulfide

Before we can calculate the mass of silver sulfide, we need to know its molar mass. The molar mass is the mass of one mole of a substance, and it's expressed in grams per mole (g/mol). To find the molar mass of silver sulfide (Ag₂S), we need to use the periodic table. We'll look up the atomic masses of silver (Ag) and sulfur (S) and then add them up, taking into account the number of atoms of each element in the compound. Think of the molar mass as the "weight" of a single mole of the substance – just like you might weigh a dozen eggs, we're weighing a mole of silver sulfide molecules!

• Atomic mass of Silver (Ag): 107.87 g/mol (approximately)
• Atomic mass of Sulfur (S): 32.07 g/mol (approximately)

Now, let's calculate the molar mass of Ag₂S:

Molar mass of Ag₂S = (2 * Atomic mass of Ag) + (1 * Atomic mass of S) Molar mass of Ag₂S = (2 * 107.87 g/mol) + (1 * 32.07 g/mol) Molar mass of Ag₂S = 215.74 g/mol + 32.07 g/mol Molar mass of Ag₂S = 247.81 g/mol

So, the molar mass of silver sulfide (Ag₂S) is approximately 247.81 grams per mole. This means that one mole of silver sulfide weighs 247.81 grams. This value is essential for our final calculation, where we'll convert moles of silver sulfide to grams.

Key Points

• Use the Periodic Table: We used the periodic table to find the atomic masses of silver and sulfur.
• Consider the Chemical Formula: We multiplied the atomic mass of silver by 2 because there are two silver atoms in Ag₂S.
• Calculate Total Molar Mass: We added the masses of all the atoms to find the molar mass of the compound.

Calculating the Mass of Silver Sulfide

We're almost there, guys! Now that we know the moles of silver sulfide formed (0.3 moles) and the molar mass of silver sulfide (247.81 g/mol), we can finally calculate the mass of silver sulfide produced. This is the final step in our stoichiometric journey, and it's where everything comes together. We'll use a simple formula to convert moles to grams:

Mass = Moles * Molar mass

Let's plug in the values we've calculated:

Mass of Ag₂S = 0.3 moles * 247.81 g/mol Mass of Ag₂S = 74.343 g

Therefore, the mass of silver sulfide formed from the reaction of sulfur with 0.6 moles of silver is approximately 74.343 grams. We've successfully navigated the stoichiometry, guys! From understanding the balanced equation to calculating moles and molar mass, we've covered all the essential steps.

Summary of the Calculation

1. Moles of Ag₂S: 0.3 moles
2. Molar mass of Ag₂S: 247.81 g/mol
3. Mass of Ag₂S: 0.3 moles * 247.81 g/mol = 74.343 g

Conclusion

So, there you have it! We've successfully calculated that approximately 74.343 grams of silver sulfide are formed from the reaction of sulfur with 0.6 moles of silver. This problem is a great example of how stoichiometry can be used to predict the amount of product formed in a chemical reaction. Remember, guys, understanding these concepts is crucial for success in chemistry. By breaking down the problem into smaller steps and focusing on the key principles, we were able to arrive at the correct answer. Keep practicing, and you'll become stoichiometry masters in no time! Chemistry can be challenging, but with a systematic approach and a good grasp of the fundamentals, you can conquer any problem that comes your way. Now, go forth and apply your newfound knowledge to other exciting chemical challenges!

This exercise highlights the importance of balanced chemical equations, molar ratios, and molar masses in stoichiometric calculations. Understanding these concepts allows us to accurately predict the outcomes of chemical reactions. Keep practicing, and you'll become a pro at solving these types of problems!