How many phosphorus atoms are in a 0.3352 g sample of Ca3(PO4)2 ?
well since nobody helped you yet I can probably get you started.
avogadro's number =6.022 × 10^23
this is the number of atoms in 1mol
you'd have to first use the grams and find the molecular weight of the compound. Ca3(PO4)2 = ?g
0.3352g ( 1mol Ca3(PO4)2 / mol weight of Ca3(PO4)2 ) = mol Ca3(PO4)2
then find out how many moles of P you have by multiplying the
(mol Ca3(PO4)2) (# mol P / 1mol Ca3(PO4)2) = # mol P
then use that and multiply that by avogadro's number to find the atoms of P you have..
#mol P (6.022*10^23 atom/ 1mol)= atoms of P
If I remember general chem correctly this should be it.
That's it, thanks.
Remember Rog, that the number of P per mole of Calcium phosphate is 2 mole P per mole of calcium phosphate.
To find the number of phosphorus (P) atoms in a sample of Ca3(PO4)2, we need to use the molar mass and Avogadro's number.
1. First, find the molar mass of Ca3(PO4)2:
- The molar mass of Ca is 40.08 g/mol.
- The molar mass of P is 30.97 g/mol.
- The molar mass of O is 16.00 g/mol.
Therefore, the molar mass of Ca3(PO4)2 is:
(3 * 40.08 g/mol) + (2 * (30.97 g/mol + 4 * 16.00 g/mol)) = 310.18 g/mol.
2. Convert the mass of the sample to moles:
Moles = Mass / Molar mass.
Moles = 0.3352 g / 310.18 g/mol.
Moles = 0.0010802 mol.
3. In the formula Ca3(PO4)2, there are two phosphorus (P) atoms.
Therefore, multiply the number of moles by 2 to find the number of phosphorus atoms:
Phosphorus atoms = 0.0010802 mol * 2.
Phosphorus atoms = 0.0021604 mol.
4. Finally, convert the number of moles to atoms using Avogadro's number:
1 mole of any substance contains 6.022 x 10^23 atoms.
Phosphorus atoms = 0.0021604 mol * 6.022 x 10^23 atoms/mol.
Phosphorus atoms = 1.303 x 10^21 atoms.
Therefore, there are approximately 1.303 x 10^21 phosphorus atoms in a 0.3352 g sample of Ca3(PO4)2.
To determine the number of phosphorus atoms in a given sample of Ca3(PO4)2, we need to use the concept of moles and Avogadro's number.
1. Calculate the molar mass of Ca3(PO4)2:
- The molar mass of one calcium atom (Ca) is 40.08 g/mol.
- The molar mass of one phosphorus atom (P) is 30.97 g/mol.
- The molar mass of four oxygen atoms (O) is 16.00 g/mol * 4 = 64.00 g/mol.
- The molar mass of one phosphate group (PO4) is 30.97 g/mol + 64.00 g/mol = 94.97 g/mol.
- Since Ca3(PO4)2 has three calcium atoms, the molar mass is 3 * 40.08 g/mol + 2 * 94.97 g/mol = 310.18 g/mol.
2. Convert the mass of the sample to moles:
- Use the equation: Moles = Mass / Molar mass.
- Moles = 0.3352 g / 310.18 g/mol ≈ 0.00108 mol.
3. Determine the number of moles of phosphorus atoms:
- From the chemical formula Ca3(PO4)2, we know that there are two moles of phosphorus atoms in one mole of Ca3(PO4)2.
- Therefore, the number of moles of phosphorus atoms = 2 * 0.00108 mol = 0.00216 mol.
4. Use Avogadro's number to calculate the number of phosphorus atoms:
- Avogadro's number is approximately 6.022 * 10^23.
- Number of phosphorus atoms = Moles of phosphorus atoms * Avogadro's number.
- Number of phosphorus atoms = 0.00216 mol * 6.022 * 10^23 ≈ 1.30 * 10^21.
Therefore, there are approximately 1.30 * 10^21 phosphorus atoms in a 0.3352 g sample of Ca3(PO4)2.