Final answer:
The average atomic mass of an element with isotopes having masses of 14, 15, and 16, with respective abundances of 95%, 3%, and 2%, is calculated to be 14.07 atomic mass units (amu).
Step-by-step explanation:
To calculate the average atomic mass of an element with multiple isotopes, we must consider the mass of each isotope and its relative abundance. In this case, the element has three isotopes with the following masses and abundances:
- Mass 14 (95% abundance)
- Mass 15 (3% abundance)
- Mass 16 (2% abundance)
The calculation involves converting the percentages into decimal fractions and then multiplying each isotope's mass by its fractional abundance. We sum these products to obtain the weighted average atomic mass:
(14 × 0.95) + (15 × 0.03) + (16 × 0.02) = 13.3 + 0.45 + 0.32 = 14.07 amu
Thus, the average atomic mass of the element is 14.07 atomic mass units (amu).