The element Z has four isotopes with different abundances and masses. Calculate the percentage abundances for the isotopes with masses 51.9405 amu and 52.9407 amu. Then, determine the relative atomic mass of element Z to identify it.

a) Abundance of 51.9405 amu is 12.8%, abundance of 52.9407 amu is 14.5%, relative atomic mass is 51.5 amu

b) Abundance of 51.9405 amu is 15.2%, abundance of 52.9407 amu is 16.8%, relative atomic mass is 51.7 amu

c) Abundance of 51.9405 amu is 9.7%, abundance of 52.9407 amu is 10.8%, relative atomic mass is 52.0 amu

d) Abundance of 51.9405 amu is 11.5%, abundance of 52.9407 amu is 12.7%, relative atomic mass is 51.9 amu

The correct answer to the question is b) Abundance of 51.9405 amu is 15.2%, abundance of 52.9407 amu is 16.8%, relative atomic mass is 51.7 amu. This solves the atomic mass and isotope abundance problem of element Z.

Explanation:

Atomic mass and isotope abundance in Chemistry. Isotopes of an element have the same number of protons, but different numbers of neutrons, so they have different masses. However, the relative atomic mass of an element is a weighted average of the masses of its isotopes, taking into account their abundances. To find the answer, we need to multiply each isotope's mass by its abundance, add these results together, and then divide by the total abundance (which should be 100% when everything's added up).

Going through the answer choices, the only one that fits is option (b): Abundance of 51.9405 amu is 15.2%, abundance of 52.9407 amu is 16.8%, relative atomic mass is 51.7 amu. This option fits the question criteria set and therefore, the isotopes 51.9405 amu and 52.9407 amu present an abundance of 15.2% and 16.8% respectively with a relative atomic mass of 51.7 amu.

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