1. For a problem I require the atomic density of uranium atoms per cm^3 in a solution of water. The atomic fraction of natural uranium to water is 1 per 100 and the net density of the solution is 1 g/cm^3. (Natural uranium is assumed to be U-235 at 0.72% of uranium atoms and the rest is U-238) (assume the atomic weights of U-235, U-238 and water are 235, 238 and 18 respectively) What I require is the atomic density of U-235 atoms, the atomic density of U 238, and H2O atoms all in atoms/cm^3. I have tried to calculate the overall atomic weight of the solution weighted by the atom concentration as in: 0.000072(235) + 0.009928(238) + 0.99(18) = 20.35 g/mol? then since the solution has net density 1 gm/cm^3: 1 / 20.35 = 0.049 mol/cm^3 then using avogadro's number convert to atoms/cm^3, then use the 1 in 100 again to find how many are U235, U238, water....is this a correct method. something seems wrong in this. thanks for the help
A simpler method is to find the mass percentages from the atomic or mole percentages that are given in the problem , then simply multiply this fraction to the solution density to find the density with respect to each substance. Then use Avogadros number to convert to the atomic density.
Assume 1 g of mixture MW U 235 X moles U 235 + MW U 238 X moles U 238 + MW H2O X moles H2O = 1 g Assume x is the moles of U 235 (x) X 9928 / 72 = moles of U 238 (x) X 990000 / 72 = moles of H2O Solve for x Then simply use Avogadros number to convert to atoms and since you found x you are able to find the moles of U 238 and H2O.