An element has only two naturally occurring isotopes. you know that isotope 1 has a mass of 44.000 amu and isotope 2 has a mass of 47.000 amu. if the average atomic mass is 45.873 amu, what are the natural abundances in percent for the two isotopes? 14.00m

isotope 1: 37.6%

isotope 2: 62.4%

Explanation:

As the element has only two naturally occurring isotopes, we can name them as:

x = mass of isotope 2; so x = 47.000amu

(1-x) = mass of isotope 1; so (1-x) = 44.000amu

Then the average atomic mass of the element must be:

Solving for x, we have:

So, with x we can find (1-x):

So, the abundance of isotope 1 is 37.6% and isotope 2 has an abundance of 62.4%.

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explanation:

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the atomic number of carbon is six, which means that a carbon atom has six protons. carbon has three naturally occurring isotopes: carbon-12, carbon-13, and carbon-14. which of these statements are true about carbon and its isotopes? select all that appl