If 2.43 grams of aluminum react with excess CuSO4, What is the theoretic yeild of Cu? And then Use the Actucal amount of Cu formed to find percent yield.You have 0.92 mass of copper metal product.
2Al + 3CuSO4 ---> Al2(SO4)3 + 3Cu
2.43 / 27 = 0.09 moles of al
0.09 x 3 / 2 x 63.5 = 8.5725 is theretical yeild
0.92/ 8.5725 x 100 = 10.73 percent
To find the theoretical yield of Cu, you need to first determine the number of moles of aluminum (Al) in 2.43 grams. The molar mass of aluminum is 27 g/mol, so dividing 2.43 grams by 27 g/mol gives you 0.09 moles of Al.
Next, you need to use the stoichiometry of the balanced chemical equation to determine the mole ratio between Al and Cu. The coefficient in front of Al is 2, and the coefficient in front of Cu is 3. This means that for every 2 moles of Al that react, 3 moles of Cu are produced.
So, you multiply the number of moles of Al by the ratio of moles of Cu to moles of Al:
0.09 moles Al x (3 moles Cu / 2 moles Al) = 0.135 moles Cu.
To convert moles of Cu to grams, you use the molar mass of copper, which is 63.5 g/mol. Therefore, 0.135 moles Cu x 63.5 g/mol = 8.5725 grams Cu.
So, the theoretical yield of Cu is 8.5725 grams.
Now, to calculate the percent yield, you need to know the actual amount of Cu formed, which is given as 0.92 grams.
To get the percent yield, divide the actual yield (0.92 grams) by the theoretical yield (8.5725 grams) and multiply by 100:
0.92 grams / 8.5725 grams x 100 = 10.73%.
Therefore, the percent yield of Cu is 10.73%.