Number of Atoms in 558.5 Grams of Iron (Fe)

In Class 11 Chemistry (Some Basic Concepts of Chemistry), the Mole Concept is crucial for calculating the number of atoms in a given mass of a substance. Let's calculate the exact number of atoms in 558.5 grams of Iron (Fe).

Question (Click to Flip)

What is the number of atoms in 558.5 gram of Fe?

Answer

The number of atoms in 558.5 grams of Fe is 6.022 × 10^24. This is calculated by dividing the mass by the atomic mass of Fe (55.85) to get 10 moles, and then multiplying by Avogadro's number.

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Key Facts

Atomic Mass of Iron (Fe): 55.85 g/mol.

Avogadro's Number: $6.022 \times 10^{23}$ atoms per mole.

Total Moles in 558.5g: 10 moles.

1. Finding the Number of Moles

To find the number of atoms, we must first find how many 'moles' of Iron we have.

Given Mass of Fe (m) = 558.5 g
Atomic Mass of Fe (M) = 55.85 g/mol (from the periodic table)

Formula: Moles (n) = Given Mass / Atomic Mass

n = 558.5 / 55.85
n = 10 moles

So, we have exactly 10 moles of Iron.

2. Using Avogadro's Number

According to Avogadro's Law, one mole of any substance contains exactly $6.022 \times 10^{23}$ particles (atoms, in this case).

Formula: Total Atoms = Number of Moles × Avogadro's Number ($N_A$)

Total Atoms = 10 × ($6.022 \times 10^{23}$)
Total Atoms = $6.022 \times 10^{24}$

Final Answer

There are $6.022 \times 10^{24}$ atoms in 558.5 grams of Iron (Fe).

Questions and Answers

What is the number of atoms in 558.5 gram of Fe?+

The number of atoms in 558.5 grams of Fe is 6.022 × 10^24. This is calculated by dividing the mass by the atomic mass of Fe (55.85) to get 10 moles, and then multiplying by Avogadro's number.

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