Question

What is the percent yield of CO2 if 46.5 grams of CO2 is recoveredfrom the reaction of 21.5 grams of C2H2 according to the reaction below?2 C2H2 + 5 O2 —> 4 CO2 + 2 H2O

Answer 1

The Percentage Yield is 63.9%

Hello

To solve this problem, we would calculate the theoritical yield of the reaction first.

Theoritical Yield

The theoritical yield of the reaction can be calculated using the equation of reaction.

Given that 2 moles of C₂H₂ will produce 4 moles of CO₂

This implies that

2*26g (from molar mass of C₂H₂) will produce 4*44g of CO₂

52g of C₂H₂ = 176g of CO₂

21.5g of C₂H₂ = xg of CO₂

cross multiply and solve for x

`\begin{gathered} x=(21.5*176)/(52) \\ x=72.77g \end{gathered}`

From the calculation above, the theoritical yield of CO₂ is 72.77g

Let's use this information and solve for the percentage yield.

Percentage Yield

This is the ratio between the actual yield to the theoritical yield and multiplied by 100.

Mathematically,

`\text{percentage yield}=\frac{actual\text{ yield}}{theoritical\text{ yield }}*100`

Data;

Actual yield = 46.5g

Theoritical yield = 72.77g

percentage yield = ?

`\begin{gathered} \text{percentage yield}=(46.5)/(72.77)*100 \\ \text{percentage yield = 63.9 \%} \end{gathered}`

From the calculations above, the Percentage Yield is 63.9%