Question

1. 0 / 1 points sulfur has four isotopes: sulfur 32 (31.97207 amu, 95.04%), sulfur 33 (32.97146 amu, 0.75%), sulfur 34 (33.96787 amu, 4.20%), sulfur 36 (35.96708 amu, 0.01%). calculate the average atomic mass for sulfur in amu and report your answer with 5 digits after the decimal. please make sure not to round until the final answer.

Explanation:

Step1: Convert percentages to decimals

$0.01\% = 0.0001$, $4.20\%=0.042$, $0.75\% = 0.0075$, $95.04\%=0.9504$

Step2: Calculate the contribution of each isotope

For sulfur - 32: $31.97207\times0.9504$
For sulfur - 33: $32.97146\times0.0075$
For sulfur - 34: $33.96787\times0.042$
For sulfur - 36: $35.96708\times0.0001$

Step3: Sum up the contributions

$31.97207\times0.9504+32.97146\times0.0075 + 33.96787\times0.042+35.96708\times0.0001$
$=31.97207\times0.9504+32.97146\times0.0075+33.96787\times0.042 + 0.003596708$
$=30.386256328+0.24728595+1.42665054+0.003596708$
$=32.063829526$

Answer:

$32.06383$