If 6.57 g of iron are reacted with an excess of hydrochloric acid, HCI, then hydrogen gas and14.63 g of iron (III) chloride are obtained. calculate the theoretical yeild and percent of yeild of FeCl3.

Well, well, well. Looks like we have some chemistry going on here. Let's break it down, shall we?

First things first, we need to find the molar mass of FeCl3. Iron (Fe) has a molar mass of 55.85 g/mol, and chlorine (Cl) has a molar mass of 35.45 g/mol (approximately). So, the molar mass of FeCl3 is: 1 iron atom (55.85 g/mol) + 3 chlorine atoms (35.45 g/mol each) = 162.26 g/mol. Got it? Good.

Now, let's convert the mass of FeCl3 obtained into moles. We have 14.63 g of FeCl3, so: 14.63 g / 162.26 g/mol = 0.090 mol of FeCl3.

Since the reaction is balanced, we can use the stoichiometry to determine the number of moles of Fe required to produce that amount of FeCl3. From the balanced equation, we see that the ratio of Fe to FeCl3 is 2:2. That means for every 2 moles of Fe, we get 2 moles of FeCl3. Therefore, we need 0.090 mol of Fe.

Now, let's calculate the molar mass of Fe. Iron (Fe) has a molar mass of 55.85 g/mol.

The theoretical yield is the amount of product that would be obtained if the reaction went to completion. So, we need to find the molar mass of Fe, then convert the moles of Fe to grams.

0.090 mol Fe x 55.85 g/mol = 5.03 g of Fe.

So, the theoretical yield of FeCl3 is 5.03 g.

To calculate the percent yield, we need the actual yield first. The actual yield is given as 14.63 g of FeCl3.

Now, we can calculate the percent yield using the formula:

Percent yield = (actual yield / theoretical yield) x 100

Percent yield = (14.63 g / 5.03 g) x 100 ≈ 290.47%

Well, isn't that something? We have a percent yield of approximately 290.47%. Looks like we got more FeCl3 than we bargained for. Maybe it's time to invest in some better clown chemistry equipment, huh? Just clowning around!

To calculate the theoretical yield and percent yield of FeCl3, we first need to determine the balanced chemical equation for the reaction between iron and hydrochloric acid (HCl):

2Fe + 6HCl -> 2FeCl3 + 3H2

From the balanced equation, we observe that the mole ratio between Fe and FeCl3 is 1:2. This means that every mole of Fe will produce 2 moles of FeCl3.

1. Calculate the moles of Fe used:
Molar mass of Fe = 55.85 g/mol
Moles of Fe = mass of Fe / molar mass of Fe
Moles of Fe = 6.57 g / 55.85 g/mol = 0.1175 mol

2. Determine the moles of FeCl3 produced:
Moles of FeCl3 = 2 * moles of Fe (from the balanced equation)
Moles of FeCl3 = 2 * 0.1175 mol = 0.235 mol

3. Calculate the theoretical yield of FeCl3:
Mass of FeCl3 = moles of FeCl3 * molar mass of FeCl3
Mass of FeCl3 = 0.235 mol * (55.85 + 3 * 35.45) g/mol
Mass of FeCl3 = 0.235 mol * 162.05 g/mol = 38.15 g

Therefore, the theoretical yield of FeCl3 is 38.15 g.

4. Calculate the percent yield of FeCl3:
Percent yield = (actual yield / theoretical yield) * 100
Percent yield = (14.63 g / 38.15 g) * 100
Percent yield = 38.3 %

Therefore, the percent yield of FeCl3 is 38.3%.

To calculate the theoretical yield and percent yield of FeCl3, you need to follow a few steps:

Step 1: Determine the balanced chemical equation for the reaction between iron (Fe) and hydrochloric acid (HCl):
2Fe + 6HCl → 2FeCl3 + 3H2

Step 2: Convert the given mass of Fe (6.57 g) to moles using the molar mass of Fe (55.845 g/mol):
Moles of Fe = Mass of Fe / Molar mass of Fe
Moles of Fe = 6.57 g / 55.845 g/mol

Step 3: Use the stoichiometry of the balanced equation to find the moles of FeCl3 produced. According to the balanced equation, 2 moles of Fe produce 2 moles of FeCl3:
Moles of FeCl3 = Moles of Fe

Step 4: Convert the moles of FeCl3 to grams using the molar mass of FeCl3 (162.204 g/mol):
Mass of FeCl3 = Moles of FeCl3 × Molar mass of FeCl3

Step 5: Calculate the theoretical yield of FeCl3 by comparing the mass of FeCl3 produced (14.63 g) with the mass calculated in Step 4:
Theoretical Yield = Mass of FeCl3 obtained / Mass of FeCl3 calculated × 100%
Theoretical Yield = 14.63 g / (Moles of FeCl3 × Molar mass of FeCl3) × 100%

Step 6: Calculate the percent yield by comparing the actual yield (14.63 g) with the theoretical yield calculated in Step 5:
Percent Yield = Actual Yield / Theoretical Yield × 100%
Percent Yield = 14.63 g / Theoretical Yield × 100%

By following these steps and using the given information, you can calculate the theoretical yield and percent yield of FeCl3.

Here is a worked example showing how to determine theoretical yield and calculate percent yield.

http://www.jiskha.com/science/chemistry/stoichiometry.html