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Element X has two isotopes. If 72.0% of the element has an isotope mass of 84.9 atomic mass units, and 28.0% of the element has an isotopic mass of 87.0 atomic mass units, the average atomic mass of element X is numerically equal to

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Answer:

Average atomic mass of an element is the sum of the masses of its isotopes each multiplied by its natural abundance

[tex]\footnotesize \longrightarrow \: \rm Average \: atomic \: mass = \dfrac{ \sum\limits \: \% age \: of \: each \: isotope \times Atomic \: mass }{100} \\ [/tex]

[tex]\footnotesize \longrightarrow \: \rm Average \: atomic \: mass = \dfrac{ 72 \times84.9 + 28 \times 87 }{100} \\ [/tex]

[tex]\footnotesize \longrightarrow \: \rm Average \: atomic \: mass = \dfrac{ 6112.8 + 2436 }{100} \\ [/tex]

[tex]\footnotesize \longrightarrow \: \rm Average \: atomic \: mass = \dfrac{ 8548.8 }{100} \\ [/tex]

[tex]\footnotesize \longrightarrow \: \bf Average \: atomic \: mass = 85.488 \: amu \\[/tex]

Cricetus

The average atomic mass will be "85.488 amu".

Given:

  • [tex]f_1 = 72[/tex]% or [tex]0.72[/tex]
  • [tex]f_2 = 28[/tex]% or [tex]0.28[/tex]
  • [tex]m_1 = 84.9 \ amu[/tex]
  • [tex]m_2 = 87 \ amu[/tex]

So,

The average atomic mass of element X will be:

= [tex](0.72\times 84.9)+(0.28\times 87)[/tex]

= [tex]61.128+24.36[/tex]

= [tex]85.488 \ amu[/tex]

Thus the above answer is correct.

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https://brainly.com/question/11065367

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