Answer:
Theoretical yield of P4O10 is 568g
Step-by-step explanation:
Step 1:
The balanced equation for the reaction. This is illustrated below:
P4(s) + 5O2(g) → P4O10(s )
Step 2:
Determination of the limiting reactant.
From the balanced equation above, 1 mole of P reacted with 5 moles of O2.
Therefore, 3 moles of P will react with = 3 x 5 = 15 moles of O2.
We can see that a higher amount of O2 than what was given is needed to react with 3 moles of P. Therefore, O2 is the limiting reactant.
Step 3:
Determination of the theoretical yield of P4O10.
In this case the limiting reactant is used as it will produce the maximum yield of the reaction. The limiting reactant is O2. The theoretical yield of P4O10 is obtained as follow:
From the balanced equation above, 5 moles of O2 produced 1 mole P4O10.
Therefore, 10 moles of O2 will produce = (10 x 1) /5 = 2 moles of P4O10.
Next, we'll convert 2 moles of P4O10 to grams to obtain the desired result. This is illustrated below:
Number of mole of P4O10 = 2 moles
Molar Mass of P4O10 = (31x4) + (16x10 = 124 + 160 = 284g
Mass of P4O10 =?
Mass = mole x molar Mass
Mass of P4O10 = 2 x 284
Mass of P4O10 = 568g
Therefore, the theoretical yield of P4O10 is 568g.