Calculate the atomic weight of an element (X) given the following information:
26X: 26.000 amu at 0.1102 fractional abundance
28X: 28.000 amu at 0.6487 fractional abundance
29X: 29.000 amu at 0.2411 fractional abundance
What element might the above problem describe? Please enter the atomic number. For example, if it is Hydrogen, enter 1.
28.02
and the atominc number is 14
Many thanks.
Ooh, did it make you feel good getting a green tick for someone else's work?
To calculate the atomic weight of an element, you need to multiply the atomic mass of each isotope by its fractional abundance and then sum up the results.
Let's start by calculating the weighted atomic mass for each isotope:
For 26X: Multiplying 26.000 amu by 0.1102 fractional abundance gives us 2.8732 amu.
For 28X: Multiplying 28.000 amu by 0.6487 fractional abundance gives us 18.1236 amu.
For 29X: Multiplying 29.000 amu by 0.2411 fractional abundance gives us 6.9999 amu.
Next, add up the weighted atomic masses of all the isotopes:
2.8732 amu + 18.1236 amu + 6.9999 amu = 27.9967 amu
Based on this calculation, the atomic weight of element X is approximately 27.9967 amu.
To determine the element, we need to find an element with an atomic weight close to 27.9967 amu. In this case, the element X corresponds to Cobalt (Co) with an atomic number of 27.