Grams (Mass) Chemistry Example 3

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Example 3

medium
What mass in grams of iron is needed to provide 2.00×10242.00 \times 10^{24} atoms of iron? (Fe = 55.85 g/mol55.85\,\text{g/mol})

Solution

  1. 1
    Convert atoms to moles: n=2.00×10246.022×1023=3.32 moln = \frac{2.00 \times 10^{24}}{6.022 \times 10^{23}} = 3.32\,\text{mol}.
  2. 2
    Convert moles to grams: m=3.32×55.85=185 gm = 3.32 \times 55.85 = 185\,\text{g}.

Answer

185 g of Fe185\,\text{g of Fe}
This reverse conversion (atoms → moles → grams) follows the same pathway but in the opposite direction. Dividing by Avogadro's number gives moles, then multiplying by molar mass gives grams.

About Grams (Mass)

A gram (g) is the fundamental unit of mass in chemistry, defined as one thousandth of a kilogram.

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More Grams (Mass) Examples

Example 1 easy

Convert [formula] moles of sodium chloride (NaCl) to grams. (Molar mass of NaCl = [formula])

Example 2 medium

How many moles are in [formula] g of sulfuric acid ([formula])? How many molecules does this represe

Example 4 hard

In the reaction [formula], calculate the mass in grams of [formula] produced from [formula] g of alu

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Related Concepts

MoleMolar Mass