Exercise 2 Natural copper is composed of two different isotopes. Their masses are 62.929 and 64.92 , respectively. The stomic number of copper is Z=29 2. Give the composition of the two isotopes. b. Knowing that the atomic mass of the natural mixture of the two isotopes is 6354, calculate the abundance of each isotope.

Let's denote the abundance of the isotope with mass 62.929 as x and the abundance of the isotope with mass 64.92 as (1-x) since the total abundance of the two isotopes is 100%.<br /><br />The atomic mass of the natural mixture can be calculated using the formula:<br /><br />Atomic mass = (mass of isotope 1 * abundance of isotope 1) + (mass of isotope 2 * abundance of isotope 2)<br /><br />Given that the atomic mass of the natural mixture is 63.54, we can set up the equation:<br /><br />63.54 = (62.929 * x) + (64.92 * (1-x))<br /><br />Solving for x, we get:<br /><br />63.54 = 62.929x + 64.92 - 64.92x<br /><br />63.54 - 64.92 = -1.973x<br /><br />-1.372 = -1.973x<br /><br />x = 1.973 / 1.973<br /><br />x = 1<br /><br />Therefore, the abundance of the isotope with mass 62.929 is 100%, and the abundance of the isotope with mass 64.92 is 0%.