A student calculates the atomic mass of sulfur to be 32.05 amu. His teacher reviews the student's work and suggests that he also account for sulfur-36, a very rare isotope that has atoms of mass 35.967 amu. By accounting for sulfur-36, how will the student's new calculation of atomic mass compare to the original calculation?
It will increase very slightly, if at all.
It will increase by about 1 or 2 amu.
It will decrease by about 1 or 2 amu.
It will increase by about 3 or 4 amu.
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A student calculates the atomic mass of sulfur to be 32.05 amu. His teacher reviews the student's wo...
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