Grams (Mass) Chemistry Example 2

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Example 2

medium
How many moles are in 49.049.0 g of sulfuric acid (H2SO4\text{H}_2\text{SO}_4)? How many molecules does this represent? (Molar mass = 98.09 g/mol98.09\,\text{g/mol})

Solution

  1. 1
    Moles: n=mM=49.098.09=0.500 moln = \frac{m}{M} = \frac{49.0}{98.09} = 0.500\,\text{mol}.
  2. 2
    Number of molecules =0.500×6.022×1023=3.01×1023= 0.500 \times 6.022 \times 10^{23} = 3.01 \times 10^{23} molecules.
  3. 3
    This chain of conversions (grams → moles → molecules) is a fundamental skill in chemistry.

Answer

0.500 mol,  3.01×1023 molecules0.500\,\text{mol},\; 3.01 \times 10^{23}\text{ molecules}
The pathway from grams to molecules always passes through moles. Molar mass connects grams to moles, and Avogadro's number connects moles to individual particles.

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 3 medium

What mass in grams of iron is needed to provide [formula] atoms of iron? (Fe = [formula])

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