Using a highly advanced mass spectrometer, a single atom of a newly discovered heavy elemental isoto — Mole Concept and Some Basic Concepts of Chemistry Chemistry Question
Question
Using a highly advanced mass spectrometer, a single atom of a newly discovered heavy elemental isotope is found to weigh exactly $3.98 \times 10^{-23}\text{ g}$. Based on this absolute mass, what is its approximate relative atomic mass on the standard macroscopic periodic table?
💡 Solution & Explanation
Step 1: Understand the relationship between absolute atomic mass and relative atomic mass. The relative atomic mass (in atomic mass units, u, or g/mol for 1 mole) is calculated by multiplying the absolute mass of a single atom by Avogadro's constant ($N_A$), because a mole is defined as $N_A$ particles. Step 2: Perform the multiplication. Atomic Mass = $\text{Mass of 1 atom} \times N_A$. Atomic Mass = $(3.98 \times 10^{-23}\text{ g/atom}) \times (6.022 \times 10^{23}\text{ atoms/mol})$. Step 3: Evaluate the result. Atomic Mass $\approx 23.96\text{ g/mol}$, which is approximately $24\text{ u}$.