Answer:
84.86%
Explanation:
Step 1:
We'll begin by writing a balanced equation for the reaction between C8H18 and O2 to produce CO2. This is illustrated below:
2C8H18 + 25O2 —> 16CO2 + 18H2O
Step 2:
Now, let us calculate the mass of O2 that reacted and the mass of CO2 produced from the balanced equation above. This is illustrated below:
Molar Mass of O2 = 16x2 = 32g/mol
Mass of O2 from the balanced equation = 25 x 32 = 800g
Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol
Mass of CO2 from the balanced equation = 16 x 44 = 704g
Therefore the mass of O2 that reacted from the balanced equation is 800g
The mass of CO2 produced from the balanced equation is 704g
Step 3:
Determination of the theoretical yield of CO2. This is illustrated below:
From the balanced equation above,
800g of O2 reacted to produced 704g of CO2.
Therefore, 218g of O2 will react to produce = (218 x 704)/800 = 191.84g of CO2.
Therefore, the theoretical yield of CO2 is 191.84g
Step 4:
Determination of the percentage yield of CO2. This is illustrated below:
Actual yield = 162.8g
Theoretical yield = 191.84g
Percentage yield =?
Percentage yield = Actual yieldm/Theoretical yield x100
Percentage yield = 162.8/191.84 x100
Percentage yield = 84.86%
Therefore, the percentage yield of CO2 is 84.86%
