Respuesta :
Answer:
To calculate the percent yield for a reaction, we need to compare the actual yield with the theoretical yield and then express this as a percentage.
Given reaction: \( \text{Al}_2\text{O}_3 + 3\text{C} \rightarrow 2\text{Al} + 3\text{CO} \)
Assuming we conducted the reaction and obtained some amount of aluminum, we would compare it to the theoretical yield we would expect based on stoichiometry and then calculate the percent yield.
Let's say we obtained 50 grams of aluminum (Al). First, we need to find the theoretical yield of aluminum using stoichiometry.
1. Calculate the molar mass of Al:
\( \text{Molar mass of Al} = 26.98 \, \text{g/mol} \)
2. Convert the mass of Al to moles:
\( \text{Moles of Al} = \frac{\text{Mass of Al}}{\text{Molar mass of Al}} = \frac{50 \, \text{g}}{26.98 \, \text{g/mol}} \)
3. Use the stoichiometric coefficients from the balanced equation to find the moles of Al2O3 required to produce the moles of Al:
From the equation, 2 moles of Al are produced from 1 mole of Al2O3.
So, moles of Al2O3 required = \(\frac{\text{Moles of Al}}{2}\)
4. Now, we'll use the stoichiometry to find the theoretical yield of Al2O3:
\( \text{Theoretical yield of Al2O3} = \text{Moles of Al2O3 required} \times \text{Molar mass of Al2O3} \)
5. Once we have the theoretical yield, we can calculate the percent yield using the formula:
\( \text{Percent yield} = \frac{\text{Actual yield}}{\text{Theoretical yield}} \times 100\% \)
If you provide the actual yield of aluminum or any other relevant information, I can help you with the calculation.
