Question

Element X has two isotopes. The table gives information about these isotopes.

Isotope Atomic Mass (amu) Abundance (%)
X-63 62.9296 69.15
X-65 64.9278 30.85
The average atomic mass of element X is
amu.

Answer 1

Answer:

                    Average Atomic Mass  =  63.5460 amu

Explanation:

Data Given:

                      Atomic Mass of ⁶³X  =  62.9296 amu

                      Natural Abundance of ⁶³X  =  69.15 %

                      Atomic Mass of ⁶⁵X  =  64.9278 amu

                      Natural Abundance of ⁶⁵X  =  30.85 %

Formula Used:

Average Atomic Mass  =  [(Atomic Mass of ⁶³X × Natural Abundance of ⁶³X) + (Atomic Mass of ⁶⁵X × Natural Abundance of ⁶⁵X)] ÷ 100

Putting values,

Average Atomic Mass  =  [(62.9296 × 69.15) + (64.9278 × 30.85)] ÷ 100

Average Atomic Mass  =  [(4351.5818) + (2003.0226)] ÷ 100

Average Atomic Mass  =  6354.6044 ÷ 100

Average Atomic Mass  =  63.5460 amu

Answer 2

Answer:

63.55

Explanation:

This is just the rounded version of the answer above. The first person is correct.

The blank wants the answer rounded the the nearest hundredth