To find the atomic mass of uranium, you can refer to the periodic table or consult reliable sources such as scientific databases or textbooks. The atomic mass of an element represents the weighted average of the masses of its naturally occurring isotopes, taking into account their relative abundances.
For uranium, there are three naturally occurring isotopes: uranium-238 (^238U), uranium-235 (^235U), and uranium-234 (^234U). These isotopes have different masses and abundances.
Uranium-238 (^238U) is the most abundant isotope of uranium and makes up approximately 99.27% of natural uranium. Its atomic mass is approximately 238.03 unified atomic mass units (u).
Uranium-235 (^235U) is a less abundant isotope and constitutes about 0.72% of natural uranium. Its atomic mass is approximately 235.04 u.
Uranium-234 (^234U) is a trace isotope found in very small quantities in natural uranium. Its atomic mass is approximately 234.04 u.
To calculate the atomic mass of uranium, you need to multiply the atomic mass of each isotope by its relative abundance (expressed as a decimal) and sum up the results. Here's an example calculation:
Atomic Mass of Uranium = (238.03 u * 0.9927) + (235.04 u * 0.0072) + (234.04 u * trace abundance of ^234U)
The precise value of the atomic mass may vary slightly depending on the updated measurements and data sources used. It's recommended to refer to reputable scientific references for the most accurate and up-to-date atomic mass values.