A naturally occurring sample of an element contains only two isotopes. The first isotope has a mass of 68.9255 amu and a natural abundance of 60.11%. The second isotope has a mass of 70.9247 amu. Determine the atomic mass of the element.

The atomic mass of copper is 63.546 amu. Do any copper isotopes have an exact mass of 63.546 amu? Explain.

An element has two naturally occurring isotopes. Isotope 1 has a mass of 120.9038 amu and a relative abundance of 57.4%, and isotope 2 has a mass of 122.9042 amu with a relative abundance of 42.6%. Calculate the atomic mass of this element and identify it.

An element has two naturally occurring isotopes. One has an abundance of 37.40% and an isotopic mass of 184.953 amu, and the other has an abundance of 62.60% and a mass of 186.956 amu. What is the average atomic mass of the element?

Calculate the atomic mass of element X given its isotopes X-45 with a mass of 44.8776 amu and 32.88% abundance, and X-47 with a mass of 46.9443 amu and 67.12% abundance.

Calculate the average mass, in grams, of one platinum atom given that the atomic mass of platinum is approximately 195.08 amu.