Question

challenge question:
while traveling to a distant universe, you discover the element \x.\ then, you discover that it is made of two isotopes, x - 23 and x - 25. to help your science team, you send the following drawing. in addition, you inform the team that the \black\ atoms are x - 23 and have an isotopic mass of 23.02 amu. the \white\ atoms are x - 25 and have an isotopic mass of 25.147 amu.
which isotope mass should the average be closest to?
what is the average atomic mass of element x?

Explanation:

Step1: Contar el número de átomos de cada isótopo

Hay 16 átomos de X - 23 y 4 átomos de X - 25. El total de átomos es \(16 + 4=20\).

Step2: Calcular la fracción de abundancia de cada isótopo

La fracción de abundancia de X - 23 es \(\frac{16}{20}=0.8\).
La fracción de abundancia de X - 25 es \(\frac{4}{20}=0.2\).

Step3: Calcular la masa atómica promedio

La masa atómica promedio \(M\) se calcula usando la fórmula \(M=(m_1\times f_1)+(m_2\times f_2)\), donde \(m_1 = 23.02\) amu, \(f_1 = 0.8\), \(m_2=25.147\) amu y \(f_2 = 0.2\).

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Answer:

La masa atómica promedio del elemento \(X\) es aproximadamente \(23.45\) amu.