Final answer:
To determine the number of moles of O₂ required to react completely with 4.0 mol of C₇H₁₆, set up a proportion using the balanced equation for the combustion of heptane.
Step-by-step explanation:
To determine the number of moles of O₂ required to react completely with 4.0 mol of C₇H₁₆, we need to examine the balanced equation for the combustion of heptane:
C₇H₁₆(g) + βO₂(g) → γCO₂(g) + H₂O(g)
From the balanced equation, we can see that the coefficient of O₂ is β. Since the ratio of C₇H₁₆ to O₂ is 1:β, we can set up a proportion :
C₇H₁₆/β = 4.0 mol/x
Solving for x, we find that x = 4.0 mol * β
So, the number of moles of O₂ required is 4.0 mol * β.
The question involves determining the number of moles of O₂ required to completely react with 4.0 mol of C₇H₁₆ in a combustion reaction. The reaction is balanced in the following way: C₇H₁₆ + 11O₂ → 7CO₂ + 8H₂O.
To balance the oxygen atoms, we multiply the number of O₂ molecules by 11 because there are a total of 22 oxygen atoms required on the product side (7 CO₂ molecules each containing 2 oxygen atoms, plus 8 H₂O molecules each containing one oxygen atom).
If 1 mol of C₇H₁₆ requires 11 mol of O₂, then 4.0 mol of C₇H₁₆ will need 4 times as much. Therefore, 4.0 mol of C₇H₁₆ will react completely with 44.0 mol of O₂.