What mass of phosphorus will be needed to produce 5.25 mol of P4O10? 4P + 5O2→ P4O10
This problem is worked the same way as the Mg(OH)2 and HCl problem just below. Post your work if you have further questions or explain fully what you don't understand.
To determine the mass of phosphorus needed to produce 5.25 mol of P4O10, we need to use the balanced chemical equation and the molar mass of phosphorus.
First, let's determine the molar mass of P4O10. P4O10 is composed of four phosphorus atoms (P) and ten oxygen atoms (O). The molar masses are:
Molar mass of P = 31.0 g/mol
Molar mass of O = 16.0 g/mol
Now we can calculate the molar mass of P4O10:
Molar mass of P4O10 = (4 x Molar mass of P) + (10 x Molar mass of O)
Molar mass of P4O10 = (4 x 31.0 g/mol) + (10 x 16.0 g/mol)
Molar mass of P4O10 = 124.0 g/mol + 160.0 g/mol
Molar mass of P4O10 = 284.0 g/mol
According to the balanced chemical equation, 1 mol of P4O10 is formed from 4 mol of phosphorus (P). Therefore, we can set up a ratio:
4 mol of P --> 1 mol of P4O10
Now, we can use this ratio to find the amount of phosphorus needed:
5.25 mol of P4O10 x (4 mol of P / 1 mol of P4O10) = 21.0 mol of P
Finally, we can convert the molar mass of phosphorus to get the mass:
Mass of P = 21.0 mol of P x molar mass of P
Mass of P = 21.0 mol x 31.0 g/mol
Mass of P = 651.0 g
Therefore, approximately 651.0 grams of phosphorus will be needed to produce 5.25 mol of P4O10.