a 4.000grams sample of aluminum metal is added to a solution containing 5.000grams of dissolved iron chloride. the reaction results in the formation of aluminum chloride and metallic iron. when the reaction is complete, unreacted aluminum remains, and this unreacted aluminum is consumed by reaction with excess hydrochloric acid. the resulting solution was decanted off and the deposited Fe metal was washed several times with water. the wet Fe was transferred to a clean, dry evaporating dish, which weighted 30.7310grams. after carefully evaporating the water, the dish and the iron residue was found to weigh 32.9150grams.
what is the balanced chemical equation and how do you find the percent yield of iron in the experiment?
I worked this for you about 4-5 hours ago.
To find the balanced chemical equation, we first need to determine the reactants and products involved in the reaction.
From the given information, we can identify the reactants:
1. Aluminum metal (Al)
2. Iron chloride (FeCl3)
The products formed are:
1. Aluminum chloride (AlCl3)
2. Metallic iron (Fe)
The balanced chemical equation for the reaction can be written as follows:
2 Al + 3 FeCl3 → 2 AlCl3 + 3 Fe
To find the percent yield of iron in the experiment, we need to compare the actual yield (experimental result) with the theoretical yield (expected result).
1. Calculate the theoretical yield of iron (Fe) using stoichiometry:
From the balanced equation, we can see that the molar ratio between Al and Fe is 2:3. Thus, the moles of Fe can be determined by converting the moles of Al:
Given mass of Al = 4.000 grams
Molar mass of Al = 26.98 g/mol (from the periodic table)
Moles of Al = given mass / molar mass = 4.000 g / 26.98 g/mol
Using the balanced equation, we can determine the moles of Fe:
Moles of Fe = (moles of Al) x (3 moles of Fe / 2 moles of Al)
2. Calculate the theoretical mass of Fe using the molar mass of Fe:
Molar mass of Fe = 55.85 g/mol (from the periodic table)
Theoretical mass of Fe = moles of Fe x molar mass of Fe
3. Calculate the percent yield using the experimental and theoretical values:
Percent Yield = (actual yield / theoretical yield) x 100
Actual yield: The mass of Fe obtained from the experiment is given as 32.9150 grams.
Theoretical yield: The calculated mass of Fe using the stoichiometry and molar mass.
Percent Yield = (Actual yield / Theoretical yield) x 100
By substituting the values, you will obtain the percent yield of iron in the experiment.