Answer:
The maximum mass of carbon dioxide, CO₂ produced is 2.64 g
Explanation:
We'll begin by writing the balanced equation for the reaction. This is illustrated below:
2C₈H₁₈ + 25O₂ —> 16CO₂ + 18H₂O
Next, we shall determine the masses of C₈H₁₈ and O₂ that reacted and the mass of CO₂ produced from the balanced equation. This can be obtained as follow:
Molar mass of C₈H₁₈ = (8×12) + (18×1)
= 96 + 18
= 114 g/mol
Mass of C₈H₁₈ from the balanced equation = 2 × 114 = 228 g
Molar mass of O₂ = 2 × 16 = 32 g/mol
Mass of O₂ from the balanced equation = 25 × 32 = 800 g
Molar mass of CO₂ = 12 + (2×16)
= 12 + 32
= 44 g/mol
Mass of CO₂ from the balanced equation = 16 × 44 = 704 g
SUMMARY:
From the balanced equation above,
228 g of C₈H₁₈ reacted with 800 g of O₂ to produce 704 g of CO₂.
Next, we shall determine the limiting reactant. This can be obtained as follow:
From the balanced equation above,
228 g of C₈H₁₈ reacted with 800 g of O₂.
Therefore, 3.43 g of C₈H₁₈ will react with = (3.43 × 800)/228 = 12.04 of O₂
From the calculations made above, we can see that a higher mass (i.e 12.04 g) of O₂ than what was given (i.e 3 g) is needed to react completely with 3.43 g of C₈H₁₈. Therefore, O₂ is the limiting reactant and C₈H₁₈ is the excess reactant.
Finally, we shall determine the maximum mass of carbon dioxide, CO₂ produced from the reaction.
To obtain the maximum mass of carbon dioxide, CO₂ produced, the limiting reactant will be used because all of it is consumed in the reaction.
The limiting reactant is O₂ and the maximum mass of carbon dioxide, CO₂ produced can be obtained as follow:
From the balanced equation above,
800 g of O₂ reacted to produce 704 g of CO₂.
Therefore, 3 g of O₂ will react to produce = (3 × 704)/800 = 2.64 g of CO₂.
Thus, the maximum mass of carbon dioxide, CO₂ produced is 2.64 g
