But your calculation treated it as 5%.lcr2139 said:Yes, I really meant 0.05%.
haruspex said:But your calculation treated it as 5%.
I believe you will also need the atomic mass of chromium.
The 0.5*10-3 was quoted as a decay rate, with the right units for that, which has nothing to do with the problem. (In fact, lcr wrote 103, not 10-3., but minus seems more likely for a decay rate.)ChuckB said:0.5*10^-3 = .0005 which = .05%
lcr2139 treated it properly in the calculation (not to say that I have any idea what the calculation is, only that I know that 0.5*10^-3 = .05%)
lcr2139 said:density of ruby = 4.02 g/cm^3
density of chromium = (4.02)(0.05) = .201 g/cm^3
Your calculation looks right to me.lcr2139 said:density of ruby: 4.02 g/cm^3
molecular weight of chromium: 52 g/mol
(4.02g/cm^3)*(.0005)*(6.022*10^23 atoms/mol) / (52 g/mol) = 2.32*10^19 cm^-3
This is wrong! The real answer is NsubT= 1.6 * 10^19 cm^-3
where am I going wrong?
The density of chromium ions in ruby is approximately 3.98 g/cm^3.
The density of chromium ions in ruby is calculated by dividing the mass of chromium ions in a given volume of ruby by the volume of the ruby sample.
The density of chromium ions in ruby can be affected by temperature, pressure, and impurities in the ruby crystal structure.
The density of chromium ions in ruby is important in determining the overall quality and value of a ruby gemstone. It can also provide insight into the formation and history of the ruby.
No, the density of chromium ions in ruby can vary slightly due to natural variations in the crystal structure and impurities present in the gemstone.