AgNO_3 + NaCl \rightarrow NaNO_3 + AgCl
How many moles of silver chloride are produced from 15.0 mol of silver nitrate?
A. 1.0 mol B. 15.0 mol C. 30.0 mol D. 45.0 mol
Understanding the Reaction: Silver Chloride Synthesis
Hey guys! Let's dive into the fascinating world of chemistry and explore how silver chloride (AgCl) is synthesized. This reaction is a classic example of a precipitation reaction, where two soluble compounds react to form an insoluble solid, which we call a precipitate. In this case, silver nitrate (AgNO_3) reacts with sodium chloride (NaCl) to produce sodium nitrate (NaNO_3) and silver chloride (AgCl). Silver chloride, being insoluble in water, precipitates out of the solution, making it easy to observe and isolate.
The balanced chemical equation for this reaction is:
AgNO_3 + NaCl \rightarrow NaNO_3 + AgCl
This equation tells us a lot. It shows the reactants (silver nitrate and sodium chloride) on the left side and the products (sodium nitrate and silver chloride) on the right side. The arrow indicates the direction of the reaction. Most importantly, the coefficients in front of each compound represent the stoichiometric ratios, which tell us the relative amounts of each substance involved in the reaction. In this particular reaction, all the coefficients are 1, meaning that one mole of silver nitrate reacts with one mole of sodium chloride to produce one mole of sodium nitrate and one mole of silver chloride. Understanding these mole ratios is crucial for solving stoichiometry problems, like the one we're about to tackle.
Stoichiometry: The Key to Mole Calculations
Stoichiometry, a fundamental concept in chemistry, deals with the quantitative relationships between reactants and products in chemical reactions. Think of it as the recipe book for chemical reactions. It allows us to predict how much of a product will be formed from a given amount of reactants, or how much of a reactant is needed to produce a specific amount of product. The balanced chemical equation is the foundation of stoichiometry because it provides the mole ratios needed for these calculations.
In our case, the balanced equation AgNO_3 + NaCl → NaNO_3 + AgCl reveals a simple 1:1 mole ratio between silver nitrate (AgNO_3) and silver chloride (AgCl). This means that for every one mole of silver nitrate that reacts, one mole of silver chloride is produced. This direct relationship makes our calculation straightforward. If we know the number of moles of silver nitrate, we can directly determine the number of moles of silver chloride produced. So, understanding stoichiometry is not just about balancing equations; it's about understanding the very essence of chemical reactions and how they occur on a molecular level. It's the bridge that connects the macroscopic world of grams and liters to the microscopic world of atoms and molecules.
Solving the Problem: Moles of Silver Chloride Produced
Okay, let's get down to business and solve the problem. The question asks: How many moles of silver chloride (AgCl) are produced from 15.0 moles of silver nitrate (AgNO_3)? Remember, we've already established that the reaction has a 1:1 mole ratio between AgNO_3 and AgCl. This makes our lives much easier!
Here's how we can approach this:
- Identify the given information: We are given 15.0 moles of AgNO_3.
- Identify the desired information: We want to find the number of moles of AgCl produced.
- Use the mole ratio: From the balanced equation, we know that 1 mole of AgNO_3 produces 1 mole of AgCl.
Now, we can set up a simple proportion or use a conversion factor:
Moles of AgCl = Moles of AgNO_3 × (Mole ratio of AgCl to AgNO_3)
Moles of AgCl = 15.0 moles AgNO_3 × (1 mole AgCl / 1 mole AgNO_3)
Moles of AgCl = 15.0 moles
Therefore, 15.0 moles of silver chloride are produced from 15.0 moles of silver nitrate. So, the correct answer is B. 15.0 mol. See, it's not so scary when you break it down step by step! Understanding the mole ratios from the balanced equation is the key to solving these types of problems. Once you grasp that, you're well on your way to mastering stoichiometry.
Why Other Options are Incorrect
It's just as important to understand why the other options are incorrect as it is to understand why the correct answer is correct. This helps solidify your understanding of the concepts and prevents you from making similar mistakes in the future. Let's take a quick look at why options A, C, and D are not the right answers.
- A. 1.0 mol: This answer is incorrect because it drastically underestimates the amount of silver chloride produced. It seems like it might be a confusion of the 1:1 mole ratio, perhaps thinking it means only 1 mole of AgCl can ever be produced, regardless of the amount of AgNO_3 used. Remember, the ratio applies proportionally – if you start with more reactant, you'll get more product.
- C. 30.0 mol: This answer is incorrect because it doubles the amount of AgNO_3. There's no mathematical operation in our balanced equation that would lead us to multiply the moles of AgNO_3 by 2. This might be a misinterpretation of the coefficients, but in this case, all coefficients are 1, indicating a direct 1:1 relationship.
- D. 45.0 mol: This answer is incorrect as it triples the amount of AgNO_3. Again, there's no basis for this calculation in the balanced equation or the stoichiometric principles involved. This kind of error might arise from simply guessing or applying an incorrect mathematical operation without understanding the underlying chemistry.
By understanding why these options are wrong, you reinforce your knowledge of the correct method and the concepts behind it. Always take the time to analyze your thought process and identify where you might have gone wrong – it's a powerful learning tool!
Key Takeaways: Mastering Stoichiometry
Alright guys, let's wrap things up and highlight the key takeaways from this problem. This wasn't just about finding the right answer; it was about understanding the underlying principles of stoichiometry and how to apply them. So, what are the main points we should remember?
- Balanced Chemical Equations are Your Best Friends: The balanced chemical equation is the foundation of all stoichiometric calculations. It provides the mole ratios between reactants and products, which are essential for determining the amounts of substances involved in a reaction. Always make sure your equation is balanced before you start any calculations!
- Mole Ratio is King: The mole ratio is the conversion factor that allows you to move between different substances in a chemical reaction. It tells you the relative amounts of each substance needed or produced. In our case, the 1:1 mole ratio between AgNO_3 and AgCl made the calculation straightforward.
- Step-by-Step Approach: Break down complex problems into smaller, manageable steps. Identify the given information, the desired information, and the relationships between them. This makes the problem less daunting and reduces the chance of errors.
- **Understand the
