What is the theoretical yield of acetaminophen from 4-aminophenol?

Unlocking the Mystery of Theoretical Yields: The Case of Acetaminophen

Ah, organic chemistry—the dark horse of the scientific world. Sometimes it feels like you’re deciphering hieroglyphs when all you want is a clear answer, right? Don’t worry; you’re not alone. One area that often trips students up is calculating theoretical yields, especially when stitching together the perfect formula for classic compounds like acetaminophen. So, let’s dissect the process using 4-aminophenol as our starting point. Grab your goggles, and let's get started!

What’s in a Name? 4-Aminophenol and Acetaminophen

First off, let’s chat a bit about our main players. 4-aminophenol, the raw material, is a versatile compound often used in dye production and, you guessed it, the synthesis of acetaminophen. The reality of organic chemistry is that a little magic happens when 4-aminophenol meets an acetylation agent, typically acetic anhydride or acetyl chloride, to form acetaminophen.

Now before we get lost in the chemistry jargon, let’s focus on our goal: calculating the theoretical yield of our prized product—acetaminophen. By the end of this, you’ll know exactly how to tackle questions like "Given 3.00 g of 4-aminophenol, what is the theoretical yield of acetaminophen?"

Unpacking the Balanced Equation

In the realm of organic chemistry, stoichiometry plays a critical role. Imagine having the perfect recipe but forgetting the amounts of each ingredient. Not a good scenario, right? Well, the beauty of a balanced chemical equation is that it gives you that all-important ratio. For our equation:

[

\text{C}_6\text{H}_7\text{NO} + \text{Acetic Anhydride} \rightarrow \text{C}8\text{H}{9}\text{NO}_2 + \text{Byproducts}

]

This tells us that one mole of 4-aminophenol reacts with one mole of acetic anhydride to yield one mole of acetaminophen. Spoiler alert: the stoichiometric ratio here is 1:1, which simplifies our lives a bit.

Finding Moles—Your New Best Friend

Next, you'll need to calculate the moles of 4-aminophenol present in your 3.00 g sample. Remember those high school chemistry classes? Time to dust off those formulas.

Let’s break it down step-by-step:

1. Calculate the Molar Mass of 4-Aminophenol (C6H7NO)

• Carbon (C): 12.01 g/mol × 6 = 72.06 g/mol

• Hydrogen (H): 1.008 g/mol × 7 = 7.056 g/mol

• Nitrogen (N): 14.01 g/mol × 1 = 14.01 g/mol

• Oxygen (O): 16.00 g/mol × 1 = 16.00 g/mol

Total molar mass of 4-aminophenol = 72.06 + 7.056 + 14.01 + 16.00 = 109.126 g/mol

2. Calculating Moles

Now the fun part! To find the number of moles:

[

\text{Moles of 4-aminophenol} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}}

]

Plugging in the numbers:

[

\text{Moles of 4-aminophenol} = \frac{3.00 \text{ g}}{109.126 \text{ g/mol}} \approx 0.0275 \text{ moles}

]

The Magic of Theoretical Yield

Now that we know how many moles of 4-aminophenol we have, it’s time to convert this into acetaminophen. Because our balanced equation gifts us a 1:1 ratio, the number of moles of acetaminophen produced will also be 0.0275 moles.

But, of course, we need that magical theoretical yield in grams. So let’s calculate the molar mass of acetaminophen (C8H9NO2):

• Carbon (C): 12.01 g/mol × 8 = 96.08 g/mol

• Hydrogen (H): 1.008 g/mol × 9 = 9.072 g/mol

• Nitrogen (N): 14.01 g/mol × 1 = 14.01 g/mol

• Oxygen (O): 16.00 g/mol × 2 = 32.00 g/mol

Total molar mass of acetaminophen = 96.08 + 9.072 + 14.01 + 32.00 = 151.162 g/mol

Now, using that information:

[

\text{Theoretical yield (g)} = \text{moles} \times \text{molar mass}

]

So we calculate:

[

\text{Theoretical yield} = 0.0275 \text{ moles} \times 151.162 \text{ g/mol} \approx 4.16 \text{ g}

]

And, voilà! The theoretical yield of acetaminophen from 3.00 g of 4-aminophenol is 4.16 g.

Wrapping It Up

Understanding how to calculate theoretical yield is a vital skill in organic chemistry. It’s like knowing the compass well enough that you won’t get lost navigating the stormy seas of reactions and conversions. Whether you’re on the path to creating effective pain relievers or pursuing further knowledge in the lab, mastering these calculations will serve you well.

Next time you tackle this topic, just remember the journey from 4-aminophenol to acetaminophen can be a lot clearer than it seems! So go ahead, share your newfound wisdom with your classmates or even engage in a fun debate about the uses of these compounds in our everyday lives. After all, chemistry isn’t just formulas and reactions; it’s the heart of our world. Happy experimenting!