39 A sample of sulfur consists mostly of 32S. It also contains 4.2% 34S and 2.8% 36S. No otherisotopes of sulfur are present.What is the relative atomic mass, Ar , of this sample of sulfur?A 32.1 B 32.2 C 34.0 D 34.3

To calculate the relative atomic mass (Ar) of the sample of sulfur, we need to take into account the proportions of each isotope and their respective atomic masses.

The calculation is as follows:

Ar = (percentage of isotope 1 x atomic mass of isotope 1) + (percentage of isotope 2 x atomic mass of isotope 2) + (percentage of isotope 3 x atomic mass of isotope 3)

Given that the sample consists mostly of 32S, we can assume that the remaining percentage (100% - 4.2% - 2.8% = 93%) is 32S.

So, the calculation becomes:

Ar = (93% x 32) + (4.2% x 34) + (2.8% x 36)

Remember to convert the percentages to decimals by dividing by 100:

Ar = (0.93 x 32) + (0.042 x 34) + (0.028 x 36)

Ar = 29.76 + 1.428 + 1.008 = 32.196

So, the relative atomic mass of this sample of sulfur is approximately 32.2. Therefore, the correct answer is B, 32.2.