Question

Element Y has 3 stable isotopes. One isotope has a mass of 27.977 amu and an abundance of 92.2%. The second isotope has a mass of 28.976 amu and an abundance of 4.7%. The third isotope has a mass of 29.974 amu and an abundance of 3.1%.

Answer 1

The average atomic mass of an element can be calculated by multiplying the mass of each isotope of that element by its abundance and then summing all the values. In this case, the average atomic mass of the element with 3 isotopes is 27.9768 amu.

Step-by-step explanation:

The average atomic mass of an element can be calculated by multiplying the mass of each isotope of that element by its abundance and then summing all the values. In this case, let's calculate the average atomic mass of the element with 3 isotopes:

Mass of isotope 1: 27.977 amu, Abundance: 92.2%

Mass of isotope 2: 28.976 amu, Abundance: 4.7%

Mass of isotope 3: 29.974 amu, Abundance: 3.1%

Using the formula:

Average Atomic Mass = (Mass1 * Abundance1) + (Mass2 * Abundance2) + (Mass3 * Abundance3)

Substituting the values, we get:

Average Atomic Mass = (27.977 * 92.2%) + (28.976 * 4.7%) + (29.974 * 3.1%)

By calculating this, we find that the average atomic mass of the element is 27.9768 amu.