How many chlorine atoms are contained in a 1.00 g sample of iron(III) chloride, FeCl3? Use the masses to two decimal places from the chart in the front of your text. Use the format 6.02E23 for 6.02 x 1023, or 6.02E-23 for 6.02 x 10-23,use two decimal places in your answer.

mols FeCl3 = 1.00g/molar mass.

mols Cl atoms = 3 times that.
Then mol Cl x 6.02E23 = ?

So I need to multiply 6.02E23 by 3?

No. That's the third step. (Read my answer again. It isn't that garbled.)

Step 1. mol FeCl3 = grams/molar mass
Step 2. mols Cl = 3 x step 1
Step 3. Step 2 x 6.02E23.

3.95*10^23

To determine the number of chlorine atoms in a 1.00 g sample of iron(III) chloride (FeCl3), we'll need to use the molar mass of FeCl3 and Avogadro's number.

First, let's find the molar mass of FeCl3 by summing up the atomic masses of iron (Fe) and three chlorine atoms (Cl):

Molar mass of FeCl3 = atomic mass of Fe + 3 * atomic mass of Cl

From the table (chart), you mentioned in the front of your text, find the atomic masses of Fe and Cl to two decimal places.

The atomic mass of Fe is usually 55.85 g/mol, but let's use the value from the table.

The atomic mass of Cl is usually 35.45 g/mol, but again, let's use the value from the table.

Once you have these values, calculate the molar mass of FeCl3.

Next, we'll convert the given mass of 1.00 g FeCl3 to moles using the formula:

moles = mass / molar mass

Finally, we'll multiply the number of moles by Avogadro's number (6.02 x 10^23) to find the number of chlorine atoms. Remember, there are three chlorine atoms in one molecule of FeCl3.

Now, go ahead and refer to the front of your text to find the atomic masses of Fe and Cl to determine the molar mass of FeCl3. Once you have calculated it, divide the given mass by the molar mass to find the number of moles. Multiply the number of moles by Avogadro's number and then multiply by three to account for the three chlorine atoms in one FeCl3 molecule. Finally, express your answer using two decimal places.