C7H6O3 + C4H6O3 → C9H8O4 + C2H4O2
If you start with 2.09 grams of C4H6O3 how many grams aspirin (C9H8O4) can you make?
Well, well, well, it seems like we've got a chemistry question here! Let's dive right in, shall we?
First, let's calculate the molar mass of C4H6O3. Carbon (C) has a molar mass of approximately 12.01 grams/mol, hydrogen (H) has a molar mass of roughly 1.01 grams/mol, and oxygen (O) has a molar mass of around 16.00 grams/mol. By adding up the molar masses of each element in C4H6O3 (4 carbons + 6 hydrogens + 3 oxygens), we get a total molar mass of approximately 102.09 grams/mol.
Now we can figure out the number of moles of C4H6O3 that we have. We can do this by dividing the given mass (2.09 grams) by the molar mass (102.09 grams/mol), which gives us roughly 0.0205 moles.
According to the balanced equation, the ratio between C4H6O3 and C9H8O4 is 1:1. So, if we have 0.0205 moles of C4H6O3, we'll end up with the same amount, 0.0205 moles, of C9H8O4.
To find the mass of C9H8O4, we need to multiply the number of moles (0.0205 moles) by its molar mass. The molar mass of C9H8O4 is approximately 180.16 grams/mol. So, multiplying 0.0205 moles by the molar mass gives us roughly 3.69 grams.
Therefore, starting with 2.09 grams of C4H6O3, you can create approximately 3.69 grams of aspirin (C9H8O4). Time to make some headache pills!
To answer this question, we need to calculate the molar masses of C4H6O3 (Reactant) and C9H8O4 (Product).
The molar mass of C4H6O3 (Reactant) can be calculated as:
C: 4 atoms x 12.01 g/mol = 48.04 g/mol
H: 6 atoms x 1.01 g/mol = 6.06 g/mol
O: 3 atoms x 16.00 g/mol = 48.00 g/mol
Adding these values gives the molar mass of C4H6O3 (Reactant):
48.04 g/mol + 6.06 g/mol + 48.00 g/mol = 102.10 g/mol
Now, let's calculate the number of moles of C4H6O3 (Reactant) using the given mass of 2.09 grams:
moles = mass / molar mass
moles = 2.09 g / 102.10 g/mol
moles ≈ 0.02042 mol
Based on the balanced chemical equation, we can see that the stoichiometric ratio between C4H6O3 and C9H8O4 is 1:1. This means that for every 1 mole of C4H6O3, we will get 1 mole of C9H8O4.
Since we have 0.02042 moles of C4H6O3, we can predict that we will also get 0.02042 moles of C9H8O4.
Now, let's calculate the mass of C9H8O4 (Product) using the molar mass of C9H8O4:
C: 9 atoms x 12.01 g/mol = 108.09 g/mol
H: 8 atoms x 1.01 g/mol = 8.08 g/mol
O: 4 atoms x 16.00 g/mol = 64.00 g/mol
Adding these values gives the molar mass of C9H8O4 (Product):
108.09 g/mol + 8.08 g/mol + 64.00 g/mol = 180.17 g/mol
Finally, let's calculate the mass of C9H8O4 (Product):
mass = moles x molar mass
mass = 0.02042 mol x 180.17 g/mol
mass ≈ 3.68 g
Therefore, starting with 2.09 grams of C4H6O3, you will be able to produce approximately 3.68 grams of aspirin (C9H8O4).
To calculate how many grams of aspirin (C9H8O4) you can make, we need to determine the limiting reagent in the reaction.
1. Start by finding the molar masses of the compounds involved:
- C7H6O3 (acetic anhydride): 122.12 g/mol
- C4H6O3 (acetyl salicylic acid): 138.09 g/mol
- C9H8O4 (aspirin): 180.16 g/mol
- C2H4O2 (acetic acid): 60.05 g/mol
2. Next, calculate the number of moles of C4H6O3 (acetyl salicylic acid) you have:
- Mass of C4H6O3 (acetyl salicylic acid) = 2.09 g
- Moles of C4H6O3 = Mass / Molar mass
= 2.09 g / 138.09 g/mol
≈ 0.0151 mol
3. Now, we need to determine the stoichiometry of the reaction to find the mole ratio of C4H6O3 to C9H8O4. From the balanced equation:
- 1 mole of C4H6O3 yields 1 mole of C9H8O4
- So, the mole ratio of C4H6O3 to C9H8O4 is 1:1
4. Since the mole ratio of C4H6O3 to C9H8O4 is 1:1, the number of moles of C9H8O4 (aspirin) produced will also be approximately 0.0151 moles.
5. Finally, calculate the mass of C9H8O4 using the moles and molar mass:
- Mass of C9H8O4 = Moles of C9H8O4 * Molar mass
= 0.0151 mol * 180.16 g/mol
≈ 2.72 g
Therefore, if you start with 2.09 grams of C4H6O3 (acetyl salicylic acid), you can produce approximately 2.72 grams of aspirin (C9H8O4).