Question

can someone check if i did this right?

Answer 1

An element has three naturally occurring isotopes. Use the information below to calculate the weighted average atomic mass of the element, showing both the setup and the final answer for the calculation

Isotope I has an atomic mass of 39.96 u and a percent abundance of 99.59%

Isotope II has an atomic mass of 37.96 u and a percent abundance of 0.065%

Isotope III has an atomic mass of 35.97 u and a percent abundance of 0.336%

Answer 2

In order to find the weighted average atomic mass you have to
First you change the percent to decimal
second you multiply it by the isotope for all three as you can see below that's what I did.
Lastly you add them together like so-
0.9959*39.96+0.00065*37.96+0.00336*35.97
The final answer is 39.942

Answer 3

did i do this right is there anything missing?^^^

Answer 4

abundance means the number of atoms of one isotope of an element divided by the total number of atoms in a mixture of the isotopes. calculate using that

Answer 5

can you show me?