Question

The average atomic mass of naturally occurring neon is 20.18 amu. There are two common isotopes of naturally occurring neon as indicated in the table below.

The table is divided into two column and two rows . The first column titled as “Isotope” and the second column titled as “Mass in atmospheric mass unit”. In the first row Ne hyphen20 is listed and in the same row the valueof Mass in atmospheric mass unit is given the value is 19.99. In the second row Ne hyphen 22 is listed and in the same row the valueof Mass in atmospheric mass unit is given the value is 21.99.

Using the information above, calculate the percent abundance of each isotope.

Calculate the number of Ne-22 atoms in a 12.55 g sample of naturally occurring neon.

A major line in the emission spectrum of neon corresponds to a frequency of 4.34 x 1014 s—1. Calculate the wavelength, in nanometers, of light that corresponds to this line.

In the upper atmosphere, ozone molecules decompose as they absorb ultraviolet (UV) radiation, as shown by the equation below. Ozone serves to block harmful ultraviolet radiation that comes from the Sun.

Answer 1

Answer:

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Answer 2

Answer:

91% Ne-20

9% Ne-22

Explanation:

20(x) + 22(1-x) = 20.18

20X + 22 - 22x = 20.18

-2x + 22 = 20.18

-2x = -1.82

2x = 1.82

x = 0.91