Question: An unknown element X has the following isotopes: 58X (68.00% abundant), 0X (26.00% abundant), 2X (6.00% abundant). What is the average atomic mass in

$An unknown element ( X ) has the following isotopes: ( { }^{58} X(68.00 % ) abundant), ( { }^{60} mathrm{X}left(26.00$

$Iron exists in nature as a mixture of predominantly three isotopes: ( { }_{26}^{54} mathrm{Fe}(53.94 mathrm{amu}),{ }_{26}$

An unknown element X has the following isotopes: 58X (68.00% abundant), 0X (26.00% abundant), 2X (6.00% abundant). What is the average atomic mass in amu of X? 56 26 26 26 Iron exists in nature as a mixture of predominantly three isotopes: 542Fe (53.94 amu), 5 Fe (55.93 amu), and 57 Fe (56.94 amu). If the most common isotope, 56 Fe, 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? 26

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