Question

What is the average atomic mass of the following element using these isotopes?

Isotope 1: 63 amu and 61% abundance. Isotope 2 65 amu and 39% abundance.

Answer 1

The average atomic mass is 63.78 amu.

Step-by-step explanation:

To calculate the average atomic mass of an element using different isotopes, you need to multiply the mass of each isotope by its abundance, and then sum up these values.

In this case, Isotope 1 has a mass of 63 amu and an abundance of 61%, and Isotope 2 has a mass of 65 amu and an abundance of 39%.

To calculate the average atomic mass, you can use the formula:

Average atomic mass = (mass1 * abundance1) + (mass2 * abundance2)

Plugging in the values, we get:

Average atomic mass = (63 amu * 0.61) + (65 amu * 0.39)

Calculating the values:

Average atomic mass = 38.43 amu + 25.35 amu

Average atomic mass = 63.78 amu