How many moles of C9H8O4 are in a 0.700 g tablet of aspirin?
n^C9H8O4 =??????
How many molecules of C9H8O4 are in this tablet?
N^C9H8O4 =?????
How many carbon atoms are in the tablet?
N^C =??????
Oh, don't worry, I've got just the right formula to calculate these things! It's called "Moletomoleculeiumcarbonicus"! Just kidding, there's no such formula, but I can help you with the calculations!
To find the number of moles of C9H8O4 in the tablet, we need to divide the tablet's mass (0.700 g) by its molar mass. The molar mass of C9H8O4 is approximately 180.16 g/mol. So, 0.700 g ÷ 180.16 g/mol = a funny number that I can't calculate at the moment.
To find the number of molecules of C9H8O4, we can use Avogadro's number, which is approximately 6.022 x 10^23 molecules/mol. Multiply the number of moles you got earlier by Avogadro's number to get the result!
As for the number of carbon atoms in the tablet, well, this might make you chuckle! Each molecule of C9H8O4 contains 9 carbon atoms. So, multiply the number of molecules by 9, and voila, you have your answer!
Remember to double-check my calculations, because even Clown Bots can make mistakes sometimes!
To determine the number of moles of C9H8O4 in the tablet, we need to use the molar mass of aspirin. The molar mass of C9H8O4 is calculated by adding up the atomic masses of each element present in the compound.
C: 9 x 12.01 g/mol = 108.09 g/mol
H: 8 x 1.01 g/mol = 8.08 g/mol
O: 4 x 16.00 g/mol = 64.00 g/mol
Adding these values together:
Molar mass of C9H8O4 = 108.09 g/mol + 8.08 g/mol + 64.00 g/mol = 180.17 g/mol
Now, we can calculate the number of moles of C9H8O4 in the 0.700 g tablet using the formula:
moles = mass / molar mass
moles = 0.700 g / 180.17 g/mol
moles ≈ 0.00388 mol
Therefore, there are approximately 0.00388 moles of C9H8O4 in the tablet.
To determine the number of molecules of C9H8O4 in the tablet, we can use Avogadro's number, which is approximately 6.022 x 10^23 molecules/mol.
molecules = moles x Avogadro's number
molecules = 0.00388 mol x 6.022 x 10^23 molecules/mol
molecules ≈ 2.33 x 10^21 molecules
Therefore, there are approximately 2.33 x 10^21 molecules of C9H8O4 in the tablet.
To find the number of carbon atoms present in the tablet, we can multiply the number of moles of C9H8O4 by the number of carbon atoms per molecule.
Carbon atoms = moles x number of carbon atoms per molecule
The chemical formula for aspirin (C9H8O4) indicates that there are 9 carbon atoms in each molecule of C9H8O4.
Carbon atoms = 0.00388 mol x 9
Carbon atoms ≈ 0.0349 mol
Therefore, there are approximately 0.0349 moles of carbon atoms in the tablet.
To answer these questions, we need to use the concept of moles and Avogadro's number.
First, let's determine the number of moles of C9H8O4 in the 0.700 g tablet of aspirin.
1. Find the molar mass of C9H8O4:
The molar mass of each element can be found on the periodic table.
C: 12.01 g/mol
H: 1.01 g/mol
O: 16.00 g/mol
Multiply the atomic masses by the number of atoms of each element in the formula:
(9 * 12.01 g/mol) + (8 * 1.01 g/mol) + (4 * 16.00 g/mol) = 180.16 g/mol
2. Calculate the number of moles:
Divide the mass of the tablet (0.700 g) by the molar mass of C9H8O4:
0.700 g / 180.16 g/mol = 0.0039 mol
So, there are 0.0039 moles of C9H8O4 in the 0.700 g tablet of aspirin.
Next, let's determine the number of molecules of C9H8O4 in the tablet.
3. Use Avogadro's number:
Avogadro's number (N_A) is approximately 6.022 x 10^23 molecules/mol.
Multiply the number of moles by Avogadro's number:
0.0039 mol * 6.022 x 10^23 molecules/mol = 2.35 x 10^21 molecules
Therefore, there are approximately 2.35 x 10^21 molecules of C9H8O4 in the tablet.
Finally, let's determine the number of carbon atoms in the tablet.
4. Use the mole ratio:
From the chemical formula C9H8O4, we know that there are 9 carbon atoms per molecule of C9H8O4.
Multiply the number of moles by the number of carbon atoms per mole:
0.0039 mol * 9 = 0.0351 mol
Therefore, there are 0.0351 moles of carbon atoms in the tablet.
what's the molar weight of aspirin?
atoms/molecules = moles * 6.023*10^23