How would you caculate this problem:
What is the mass in grams of 150*10^12 iron atoms, each having a mass of 56 amu?
To calculate the mass in grams of a certain number of atoms, we'll need to perform several steps:
Step 1: Determine the molar mass of iron.
The atomic mass of iron is 56 atomic mass units (amu). This means that one mole of iron atoms has a mass of 56 grams. The molar mass of iron is therefore 56 g/mol.
Step 2: Convert the given number of iron atoms to moles.
We are given the number of iron atoms as 150 * 10^12. To convert this to moles, we need to divide by Avogadro's number, which is 6.022 * 10^23 particles/mol. Let's calculate it:
150 * 10^12 / (6.022 * 10^23) mol
Step 3: Calculate the mass in grams.
Now we can use the molar mass of iron to convert the amount of substance in moles to grams. We will multiply the number of moles by the molar mass:
(150 * 10^12 / (6.022 * 10^23)) * 56 g
Perform the calculations to get the final answer:
(150 * 10^12) * 56 / (6.022 * 10^23) g
Note: The final answer may be a very small number due to the vast difference between the mass of a single atom and Avogadro's number.
I hope this explanation helps you understand how to calculate the mass in grams of a given number of atoms. Let me know if you have any further questions!