For the reaction 4FeCl2(aq) + 3O2(g) → 2Fe2O3(s) + 4Cl2(g), what volume of a 0.650 M solution of FeCl2 is required to react completely with 8.58 × 1021 molecules of O2?

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Why did the iron chloride go to the party? Because it heard there was going to be a lot of oxygen to react with!

To solve this problem, let's break it down step by step:

First, let's calculate the number of moles of O2. We know that there are 8.58 × 10^21 molecules, and since Avogadro's number tells us that 1 mole is equal to 6.022 × 10^23 molecules, we can calculate:

Number of moles of O2 = (8.58 × 10^21) / (6.022 × 10^23) = ?

Calculating this, we find that there are approximately 0.0142 moles of O2.

Now, let's use the balanced equation to find the ratio of FeCl2 to O2. From the equation, we can see that the ratio is 4:3. So for every 4 moles of FeCl2, we need 3 moles of O2.

Using this ratio, we can set up a proportion to find the number of moles of FeCl2 needed:

(4 moles FeCl2) / (3 moles O2) = x moles FeCl2 / (0.0142 moles O2)

Cross-multiplying and solving for x, we find that x ≈ 0.0189 moles of FeCl2.

Now that we know the number of moles of FeCl2 needed, we can calculate the volume of the 0.650 M solution using the formula:

Molarity = (moles of solute) / (volume of solution in liters)

Rearranging the formula to solve for volume:

Volume of solution = (moles of solute) / (Molarity)

Plugging in the values:

Volume of solution = (0.0189 moles) / (0.650 M) ≈ 0.0291 L

Converting liters to milliliters, we get:

Volume of solution ≈ 29.1 mL

So, approximately 29.1 mL of the 0.650 M solution of FeCl2 is required to react completely with 8.58 × 10^21 molecules of O2.

To answer this question, we need to use the balanced chemical equation and stoichiometry to find the number of moles of FeCl2 required to react with a given number of molecules of O2. Then, we can use the concentration of the FeCl2 solution to calculate the volume needed.

Let's break down the steps:

Step 1: Calculate the number of moles of O2
Given: 8.58 × 10^21 molecules of O2

To convert from molecules to moles, we need to divide by Avogadro's number (6.022 × 10^23 molecules/mol):
moles of O2 = (8.58 × 10^21 molecules) / (6.022 × 10^23 molecules/mol)

Step 2: Use the balanced chemical equation to find the stoichiometric ratio between O2 and FeCl2
The balanced equation is:
4FeCl2(aq) + 3O2(g) → 2Fe2O3(s) + 4Cl2(g)

From the equation, we can see that for every 3 moles of O2, we need 4 moles of FeCl2.

Step 3: Calculate the number of moles of FeCl2 required
moles of FeCl2 = (moles of O2) × (4 moles of FeCl2 / 3 moles of O2)

Step 4: Convert moles of FeCl2 to volume of the FeCl2 solution
Given: Concentration of the FeCl2 solution = 0.650 M (moles/L)

Now we can use the definition of concentration (moles/L) to calculate the volume needed:
volume of FeCl2 solution = (moles of FeCl2) / (0.650 moles/L)

This will give us the volume in liters, but if we need the answer in milliliters or any other unit, we can convert accordingly.

By following these steps, you should be able to calculate the volume of the 0.650 M solution of FeCl2 required to react completely with 8.58 × 10^21 molecules of O2.

mols O2 = 8.58E21/6.02E23 = ?

Using the coefficients in the balanced equation, convert mols O2 to mols FeCl2. That's ? mols O2 x (4 mols FeCl2/3 mols O2) = ?
Then M FeCl2 = mols FeCl2/L FeCl2. You know M and mols, solve for L