D/4214027 CHAPTERS RESOURCES PROGRESS TRAC Chapter 3-Atoms the Building Blacks o

Question

D/4214027 CHAPTERS RESOURCES PROGRESS TRAC Chapter 3-Atoms the Building Blacks of Elements Chapter 3 Review Questions Amanda Brock-Feb 21, 2018 114240 PM Return to Site (12 of 25) Calculate the atomic mass of silver if siver has 2 naturally occurmring isotopes with the followin Ag-107 106.90509 g/mol Ag-109 108.90476 g/mol g masses and natural abundances 5154% 1.1 x 10 6 022 x 1022 432.15 107.87 Skip Questien 1Am Finlshed/Submit for Brade ? For questions or concems teperdingis Heving troubles viewing something on e ll righes reserved 02002-201a MacBook Air 9

Explanation / Answer

12)

This is problem based on average atomic weight.

So, in order to calculate it, each atomic mass is multiplied by its % abundance. Then, add the results together to get the your average atomic mass, ie

Average atomic mass = atomic mass of isotope 1 x % abundance + atomic mass of isotope 2 x % abundance

Or, average atomic mass = 107 x (51.54/100) + 109(48.46 /100)

Average atomic mass = 107.97 amu

So, 4th option is the correct choice.

13)

Since, mass = molar mass x number of moles

Mass = 18 x 1.2

Mass = 21.6 g

Option 1st is the correct choice.

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