Question

1. the following table shows the mass and abundance of three isotopes of element j. which setup would calculate the average atomic mass of element j correctly? isotope a b c mass number (grams) z y w percent abundance (%) 15 50 35 15 + 50 + 35 / 3 = average atomic mass of j mass z+mass y + mass w / 3 = average atomic mass of j (mass z x 0.15)+(mass y x 0.50)+(mass w x 0.35)=average atomic mass of j (mass z + 0.15)+(mass y + 0.50)+(mass w + 0.35)=average atomic mass of j clear all

Explanation:

Step1: Recall formula for average atomic mass

The average atomic mass of an element with isotopes is calculated by multiplying the mass of each isotope by its percent - abundance (expressed as a decimal) and then summing these products.
Let the masses of the isotopes be \(W\), \(Y\), and \(Z\) with percent abundances \(35\%\), \(50\%\), and \(15\%\) respectively. The percent abundances as decimals are \(0.35\), \(0.50\), and \(0.15\).
The formula for the average atomic mass of element \(J\) is \((W\times0.35)+(Y\times0.50)+(Z\times0.15)\).

Answer:

(Mass Z x 0.15)+(Mass Y x 0.50)+(Mass W x 0.35) = Average atomic mass of J