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.

Sketch the mass spectrum of magnesium given its three naturally occurring isotopes with the following masses and natural abundances: Isotope Mass (amu) Abundance (%) - Mg-24: 23.9850, 78.99% - Mg-25: 24.9858, 10.00% - Mg-26: 25.9826, 11.01%.

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.