Question

14 select the correct answer. using the information in the table, what is the average atomic mass of sulfur? isotope relative abundance (%) atomic mass (amu) s - 32 94.93 31.972 s - 33 0.76 32.971 s - 34 4.29 33.967 s - 36 0.02 35.967 a. 31.972 amu b. 32.060 amu c. 33.71 amu d. 34.090 amu e. 35.967 amu

Explanation:

Step1: Convert percentages to decimals

$94.93\% = 0.9493$, $0.76\%=0.0076$, $4.29\% = 0.0429$, $0.02\%=0.0002$

Step2: Calculate the contribution of each isotope

For S - 32: $0.9493\times31.972\approx30.353$
For S - 33: $0.0076\times32.971\approx0.250$
For S - 34: $0.0429\times33.967\approx1.457$
For S - 36: $0.0002\times35.967\approx0.007$

Step3: Sum up the contributions

$30.353 + 0.250+1.457 + 0.007=32.067\approx32.060$

Answer:

B. 32.060 amu