The average atomic mass of carbon, made up of 2 naturally occurring isotopes, 12C and 13C, is 12.01 u.
The element carbon has two naturally occurring isotopes. 12C with an atomic mass of 12.00 u and an abundance of 98.93% and 13C with an atomic mass of 13.00 u and an abundance of 1.07%. We can find the average atomic mass (aam) of carbon, which is a weighted average that considers the mass of each isotope ([tex]m_i[/tex]) and the abundance of each isotope ([tex]ab_i[/tex]) using the following expression.
[tex]aam = \frac{\Sigma m_i \times ab_i }{100} = \frac{12.00 u \times 98.93 + 13.00 \times 1.07}{100} = 12.01 u[/tex]
The average atomic mass of carbon, made up of 2 naturally occurring isotopes, 12C and 13C, is 12.01 u.
You can learn more about average atomic mass here: https://brainly.com/question/3187640
