For example, to convert the mass of one lithium atom to the mass of \( \frac{6.941 \mathrm{amv}}{\mathrm{Li} \text { atom }} \times \frac{6.022 \times 10^{23} \mathrm{Li} \text { atoms }}{1 \mathrm{~mol}} \times \frac{1}{6.022 \times 10^{23}}=6.941 \frac{\mathrm{~g}}{\mathrm{~mol}} \mathrm{Li} \) atoms.

Did you know that 6.941 g/mol is the atomic mass of lithium? This number is a key player in the periodic table, and it arises from the abundance of the isotope lithium-7, which is responsible for most lithium found in nature. Understanding atomic mass isn’t just for chemistry classes; it’s essential for everything from pharmaceuticals to creating batteries, as lithium is a vital component in rechargeable lithium-ion batteries. When converting moles to grams, a common mistake is neglecting to ensure the units cancel out appropriately. Always double-check your conversion factors! Also, be mindful that when dealing with isotopes, the atomic mass may vary slightly. It’s essential to use the correct values for precise measurements, especially in experiments where accurate dosing is critical, like in medicine or materials science.