So I think I have done this problem right, I was just wondering if anyone would check over it for me.
What mass (in grams) of P2O5 contains 1.20 x 1023 atoms of phosphorus?
1.20E23 atoms of P x (1 mol/ 6.022E23 atoms) x (5 mol O/ 2 mol P) x (1 mol P2O5/ 5 mol O) x (79.995g/ 1 mol P2O5) =
7.97g of P2O5
I don't understand why you went through the oxygen link; however, one factor canceled the other so no harm done except for extra work. The only error I see is the molar mass P2O5 should be 141.94 grams instead of 79.995.
To solve this problem, you can use dimensional analysis or conversion factors.
1. Start with the given number of atoms of phosphorus: 1.20 x 10^23 atoms of P.
2. Use Avogadro's number as a conversion factor: 1 mol/6.022 x 10^23 atoms. This will convert the number of atoms to moles.
3. Since the balanced chemical equation for P2O5 shows that there are 2 moles of P per 1 mole of P2O5, use the conversion factor: 5 mol O/2 mol P. This will convert moles of P to moles of O.
4. Continuing with the balanced chemical equation, use the conversion factor: 1 mol P2O5/5 mol O. This will convert moles of O to moles of P2O5.
5. Finally, use the molar mass of P2O5 (phosphorus pentoxide) as a conversion factor: 79.995 g/1 mol P2O5. This will convert moles of P2O5 to grams of P2O5.
By multiplying all these conversion factors together, you will get the mass of P2O5 in grams. In this case, the answer is approximately 7.97 g of P2O5.
It looks like you have correctly applied the conversion factors and arrived at the correct answer of 7.97 g of P2O5. Well done!