Question

Potassium has three naturally occurring isotopes. According to one source of data, Potassium-39 (mass 38.9637 amu) makes up 93.26%, potassium-40 (mass 39.9640 amu) makes up just 0.01%, and potassium-41 (mass 40.9618 amu) makes up 6.73%. What is the average atomic mass of potassium based on these relative abundances

Answer 1

Answer:

Average atomic mass of potassium based on these relative abundances

$= 39.0944$

Explanation:

The atomic mass of this element will be equal to the sum of product of its three isotopic masses and its fractional abundance

For isotope I -

Mass of Potassium-39 $= 38.9637$ amu

Fractional abundance of Potassium-39 $= 93.26$ %

Mass of Potassium-40 $= 39.9640$ amu

Fractional abundance of Potassium-40 $= 0.01$ %

Mass of Potassium-41 $= 40.9618$ amu

Fractional abundance of Potassium-41 $= 6.73$%

Average atomic mass of potassium based on these relative abundances

$= (38.9636 * 0.9326)+ (39.9640*0.0001) + (40.9618 * 0.0673)\\= 36.3374 + 0.0003 + 2.7567\\= 39.0944$

Answer 2

The average atomic mass of potassium based on these relative abundances is 39.0944.

Calculation of the average  atomic mass of potassium:

Since the Potassium-39 (mass 38.9637 amu) makes up 93.26%, potassium-40 (mass 39.9640 amu) makes up just 0.01%, and potassium-41 (mass 40.9618 amu) makes up 6.73%.

So,

= (38.9637 of 93.26%) + (39.9640 of 0.01%) + (40.9618 of 6.73%)

= 36.3374 + 0.0003 + 2.7567

= 39.044

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