Answer:
7.03g
Explanation:
4P + 5O2 → 2P2O5
Let us convert the mass given to mole. This can be achieved by doing the following:
Molar Mass of O2 = 16x2 = 32g/mol
Mass of O2 = 6.09g
Number of mole = Mass /Molar Mass
Number of mole of O2 = 6.09/32 = 0.19mol
Molar Mass of P = 31g/mol
Mass of P = 3.07g
Number of mole of P = 3.07/31 = 0.099mol
Let us determine the limiting reactant and the excess reactant
From the equation,
4moles of P required 5moles of O2.
Therefore, 0.099mol of P will require = (0.099 x 5)/4 = 0.12mol
From the above illustration, we see clearly that not all the O2 reacted as the number of mole of O2 obtained from the question is 0.19mol. This means that O2 is the excess reactant and P is the limiting reactant.
Note: the limiting reactant is always used to obtain the yield of any reaction.
Now we can obtain the theoretical yield of P2O5 as follows:
4P + 5O2 → 2P2O5
Molar Mass of P = 31g/mol
Mass of P from the equation = 4x31 = 124g
Molar Mass of P2O5 = (31x2) + (16x5) = 62 + 80 = 142g/mol
Mass of P2O5 from the equation = 2 x 142 = 284g
From the equation,
124g of P produced 284g of P2O5.
Therefore, 3.07g of P will produce = (3.07x284)/124 = 7.03g of P2O5.
Therefore, the theoretical yield of P2O5 is 7.03g
