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We are asked to give the atomic masses (relative atomic mass) of each of these peaks.
1H (atomic mass = 1.00783 amu)
2H (atomic mass = 2.01410 amu)
The 3 peaks observed are:
A) 1H -1H
B) 1H -2H
C) 2H -2H
Calculate relative atomic masses:
Mass spectrometry is more often applied to molecules than to atoms. We will see in Chapter 3 in the textbook that the molecular weight of a molecule is the sum of the atomic weights of the atoms in the molecule. In mass spectrometry, these molecular weights are measured relative to 1/12 the mass of one atom of 12C and therefore are commonly referred to as relative masses. The mass spectrum of H2 is taken under conditions that prevent decomposition into H atoms.
The two naturally occurring isotopes of hydrogen are 1H (atomic mass = 1.00783 amu; abundance 99.9885%) and 2H (atomic mass = 2.01410 amu; abundance 0.0115%).
Give the atomic masses (relative atomic mass) of each of these peaks.
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Based on our data, we think this problem is relevant for Professor Caldwell's class at UCONN.