This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Step 1: Identify the isotopes and their abundances. The element is Neon (Ne) with three isotopes: • ^20Ne has an isotopic mass of 20 amu and an abundance of 90.92\%. • ^21Ne has an isotopic mass of 21 amu and an abundance of 0.26\%. • ^22Ne has an isotopic mass of 22 amu and an abundance of 8.82\%. Step 2: Convert the percentage abundances to fractional abundances. • For ^20Ne: (90.92)/(100) = 0.9092 • For ^21Ne: (0.26)/(100) = 0.0026 • For ^22Ne: (8.82)/(100) = 0.0882 Step 3: Calculate the relative atomic mass using the formula: Relative Atomic Mass = (isotopic mass × fractional abundance) Relative Atomic Mass = (20 × 0.9092) + (21 × 0.0026) + (22 × 0.0882) Relative Atomic Mass = 18.184 + 0.0546 + 1.9404 Relative Atomic Mass = 20.179 The relative atomic mass of Neon is 20.179 amu. Send me the next one 📸