Oxygen, which appears in nature as O (mass = 16.00 amu), O (mass = 17.00 amu), a

Question

Oxygen, which appears in nature as O (mass = 16.00 amu), O (mass = 17.00 amu), and O (mass = 18.00 amu) has an atomic weight of 16.00 amu. Which isotope predominates? Question 18. a. How many moles of nitrogen is 1.03 x 1018 nitrogen atoms? Oxygen, which appears in nature as O (mass = 16.00 amu), O (mass = 17.00 amu), and O (mass = 18.00 amu) has an atomic weight of 16.00 amu. Which isotope predominates? Question 18. a. How many moles of nitrogen is 1.03 x 1018 nitrogen atoms? Oxygen, which appears in nature as O (mass = 16.00 amu), O (mass = 17.00 amu), and O (mass = 18.00 amu) has an atomic weight of 16.00 amu. Which isotope predominates? Question 18. a. How many moles of nitrogen is 1.03 x 1018 nitrogen atoms?

Explanation / Answer

naturally ocurring oxygen is composed of three stable isotopes 16O,17O,18O,with 16O being the most abundant(99.762% natural abundance).

the relative and absolute of 16O is high because it is a principal product of steller evolution and because it is a primary isotope, means it can be made by star that were initially made exclusively of hydrogen. Most 16O is synthesized at the end of the helium fusion process in the stars,the triple -alpha reaction creates 12C ,which captures an additional 4He to make 16O.The neon burning process creates additional 16O.

Natural isotopic aundances : 16O= 99.762%

17O=0.03755%

18O=0.1995%

answer 18(a): A mole is defined as 6.023*10^23 atoms/molecules,

so 1 atom would be a 1/6.023*10^23 fraction of a mole

so in given question: 1.023*10^18 nitrogen atom

the molecular mass of nitrogen atom=14

so, 1 mole of nitrogen=14 g * 1.03*10^18*6.023*10^23

= 86.85166*10^18*10^23

=86.85166*10^41 gmoles

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