Respuesta :
Answer:
Theoretical yield = 2.56 moles of CO₂
Explanation:
2 C₈H₁₈(l) + 25 O₂( g) → 16 CO₂( g) + 18 H₈O( g)
As per the given balanced equation 2 moles of C₈H₁₈ combines with 25 moles of O₂. So 4 moles of of C₈H₁₈ requires 50 moles of O₂. But in the given question we have 4 moles of O₂ there O₂ is the limiting reagent.
The limiting reagent determines the yield of the product. Therefore, here O₂ will determines the yield of CO₂.
As per the given balanced equation 25 moles of O₂ yields 16 moles of CO₂.
Therefore, 4 moles of O₂ will yield ([tex]\frac{16}{25}[/tex] x 4 ) moles of CO₂
= 2.56 moles of CO₂
In a chemical reaction, the maximum amount of the product that can be formed is called the theoretical yield. This along with the actual yield gives the percentage yield.
2.56 moles [tex]\rm CO_{2}[/tex] theoretical yield.
How to calculate the theoretical yield?
Given,
- Moles of [tex]\rm C_{8}H_{18}[/tex] = 4 moles
- Moles of [tex]\rm O_{2}[/tex] = 4 moles
- The molar mass of the [tex]\rm CO_{2}[/tex] = [tex]\rm 44 g/mol[/tex]
The balanced chemical reaction can be shown as,
[tex]\rm 2C_{8}H_{18} + 25 CO_{2} \rightarrow 16 CO_{2} + 18 H_{2}O[/tex]
From the reaction, it can be said that,
25 moles of oxygen reacts with 2 moles of [tex]\rm C_{8}H_{18}[/tex]
So, 4 moles of oxygen = X moles of [tex]\rm C_{8}H_{18}[/tex]
[tex]\begin{aligned}\rm X &= \dfrac{2}{25} \times 4\\\\&= 0.32\;\rm moles\end{aligned}[/tex]
From this, it can be said that oxygen is the limiting reagent.
25 moles of Oxygen = 16 moles of [tex]\rm CO_{2}[/tex]
4 moles of Oxygen = X moles of [tex]\rm CO_{2}[/tex]
[tex]\begin{aligned}\rm X &= \dfrac{16}{25}\times 4\\\\&= 2.56 \;\rm moles \end{aligned}[/tex]
Therefore, 2.56 moles of Carbon dioxide is produced.
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