this exercise will lead you to verify that the average atomic mass of magnesium is 24.31 amu, based on the…

this exercise will lead you to verify that the average atomic mass of magnesium is 24.31 amu, based on the following information: isotope mass (amu) percent abundance 24mg 23.985042 78.99% 25mg 24.985837 10.00% 26mg 25.982593 11.01% what is the value: atomic mass x fractional abundance for 25mg? for now, report your answer to three decimal places. mass contribution of 24mg = 18.946 amu (3 of 5) show approach check

this exercise will lead you to verify that the average atomic mass of magnesium is 24.31 amu, based on the following information: isotope mass (amu) percent abundance 24mg 23.985042 78.99% 25mg 24.985837 10.00% 26mg 25.982593 11.01% what is the value: atomic mass x fractional abundance for 25mg? for now, report your answer to three decimal places. mass contribution of 24mg = 18.946 amu (3 of 5) show approach check

Answer

Explanation:

Step1: Convert percent abundance to fractional abundance

For (^{24}\text{Mg}), fractional abundance (= 78.99%=0.7899); for (^{25}\text{Mg}), fractional abundance ( = 10.00% = 0.1000); for (^{26}\text{Mg}), fractional abundance (=11.01% = 0.1101)

Step2: Calculate mass - contribution of (^{25}\text{Mg})

Mass - contribution (=\text{atomic mass}\times\text{fractional abundance}). The atomic mass of (^{25}\text{Mg}) is (24.985837) amu and its fractional abundance is (0.1000). So, mass - contribution (=24.985837\times0.1000 = 2.4985837) amu

Step3: Round the result

Rounding (2.4985837) amu to three decimal places gives (2.499) amu

Answer:

(2.499) amu