The hemoglobin content of blood is about 15.4g/100mL blood. The molar mass of hemoglobin is about 64500 g/mol, and there are four iron (Fe) atoms in a hemoglobin molecule.Approximately how many Fe atoms are present in the 6 L of blood in a typical adult?

[(15.5g / 100ml]) * ([1ml / 1x10^-3 L]) * ([1Hemoglobin / 645000g Hemoglobin]) * ([4Fe / 1 hemoglobin]) * ([6.022x10^23 / 1mol])
theres something wrong and i cant figure out what it is. The answer i should be getiing is 3*10^22 but i can't get it.

Thanks for showing your work.

15.4 and not 15.4

You don't have the 6L blood . I get 3.4E22

OOO thanks

Ah, a question about blood! It seems like you're on the right track with your calculation, but there might be a small error in your conversion. Let's break it down step by step to see what's going wrong:

1. Start with 15.4 g/100mL * (6 L / 1x10^3 mL) * (1 Hemoglobin / 64500 g Hemoglobin).
This will give you the number of hemoglobin molecules in 6 liters of blood.

2. Next, multiply by the number of iron (Fe) atoms per hemoglobin molecule, which is 4 Fe / 1 hemoglobin.
This will give you the number of iron atoms.

3. Finally, multiply by Avogadro's number, 6.022x10^23 atoms/mol.
This will give you the final answer in atoms.

The correct calculation should look like this:

(15.4 g/100 mL) * (6 L / 1x10^3 mL) * (1 Hemoglobin / 64500 g Hemoglobin) * (4 Fe / 1 Hemoglobin) * (6.022x10^23 atoms / 1 mol)

By plugging in the numbers, you should indeed get approximately 3x10^22 iron atoms in 6 liters of blood from a typical adult. Keep going, you're almost there!

To find the number of Fe atoms present in 6 L of blood, we need to follow the correct steps in the calculation. Let's break down the calculation step by step:

1. Convert the hemoglobin content from grams to moles:
(15.4 g / 100 mL) * (1 mL / 1 × 10^-3 L) * (1 mol / 64500 g) = 2.393 × 10^-2 mol

2. Determine the number of hemoglobin molecules:
To find the number of hemoglobin molecules, we need to divide the number of moles by Avogadro's number (6.022 × 10^23):
2.393 × 10^-2 mol * (6.022 × 10^23 / 1 mol) = 1.442 × 10^22 molecules

3. Calculate the number of Fe atoms present in the hemoglobin molecules:
Since there are four iron (Fe) atoms in each hemoglobin molecule, multiply the number of hemoglobin molecules by 4:
1.442 × 10^22 molecules * 4 = 5.768 × 10^22 Fe atoms

So, the approximate number of Fe atoms present in 6 L of blood is 5.768 × 10^22 Fe atoms, not 3 × 10^22 Fe atoms as stated in your question. Double-check your calculations to make sure you are using the correct values for calculations.