Iron exists in nature as a mixture of predominantly three isotopes: 5426Fe (53.94 amu), 562.Fe (55.93 amu), and 5726Fe (56.94 amu). If the most common isotope, 5626Fe, accounts for 91.75% of iron atoms, and the average atomic mass of iron is 55.85 amu, what is the percent abundance of the rarest of these three isotopes of iron?

Following the ideas above, show that this data illustrates the law of multiple proportions. (Compare the masses of bromine that react with 1.00 g of gold). Two compounds of gold and bromine have these percent compositions: Compound X is 45.11% Au and 54.89% Br, Compound Y is 71.14% Au and 28.86% Br

2. A one-carat diamond has a mass of 2.00 x 10 _1 g. Assuming the diamond is made of pure carbon, determine the number of carbon atoms in a one-carat diamond.

(c) A metal has six naturally occurring isotopes. The isotopes, their fractions, and their atomic weights are presented in the table below. Calculate the average atomic weight of the metal. Fraction Atomic weight Isotope 1 0.16% 173.940 amu Isotope 2 5.26% 175.941 amu Isotope 3 18.60% 176.943 amu Isotope 4 27.28% 177.944 amu Isotope 5 13.62% 178.946 amu Isotope 6 35.08% 179.947 amu