as level chemistry isotopic mass 👍👍👍?

32x + 34(1 - x) = 32.09 =>

34 - 32.09 = 2x =>

x = 0.955.

So, it's 95.5% of the 32 isotope, and 4.5% of the 34 isotope.

Which is about right for a "natural" sample.

The average atomic weight is the weighted average of the isotopic masses.

.... atomic weight = RA1 x M1 + RA2 x M2 + RA3 x M3 ....

Where RA is the relative abundance expressed as a decimal and M is the weight of the isotope.  RA1 + RA2 + RA3 +... = 1

Since there are two isotopes represented in this question, let x = RA for S-32, and (1-x) = RA for S-34.

32.0x + (1-x)(34) = 32.09

32.0x + 34 - 34x = 32.09

-2x = -1.91

x = 0.955

The relative abundance of S-32 is 0.955, or 95.5%, and the relative abundance of S-34 is 0.045, or 4.5%.

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This question is taking some liberties with the masses of the isotopes. In addition, the average atomic weight of sulfur is 32.06 amu, not 32.09 amu. There are four stable isotopes of sulfur, but the other two have relative abundances of less that 1%. This question serves to illustrate how to deal with two isotopes.

Simple mass balance. X1*M1+x2*M2 = 1xMass total and X1+X2=1.  Simultaneous equations: two equations with two unknowns, solve it.  Substitution is the usual way (make X1=1-X2, or the reverse, X2=1-X1) and plug it in.

EDIT.  Did not expect the Christmas colors.