The relative abundances of two isotopes of ru | vedclass

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(A) The average atomic mass is calculated using the formula: $	ext{Average Atomic Mass} = \sum (	ext{Isotopic Mass} 	imes 	ext{Fractional Abundanc

Vedclass · Accepted Answer

$85$

Vedclass · Answer

(A) The average atomic mass is calculated using the formula: $	ext{Average Atomic Mass} = \sum (	ext{Isotopic Mass} 	imes 	ext{Fractional Abundance})$.Given:Isotope $1$: Mass = $85$,Abundance = $75\% = 0.75$.Isotope $2$: Mass = $87$,Abundance = $25\% = 0.25$.Calculation:$	ext{Average Atomic Mass} = (85 	imes 0.75) + (87 	imes 0.25)$$= 63.75 + 21.75$$= 85.5 	ext{ u}$.Therefore,the correct option is $A$.

The relative abundances of two isotopes of rubidium with atomic masses $85$ and $87$ are $75\%$ and $25\%$ respectively. What is the average atomic mass of rubidium (in $.5$)?

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