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238 grams/mole
The isotopic number is the approximate mass for any element. Such as if I say Carbon 14, the approximate mass is 14 grams/mole.
If you are asking what is the mass of one atom of Uranium 238:
Then you take the isotopic mass 238 grams/mole and divide by Avogadro's Number 6.022X10^23 atoms/mole this gives you units of grams/atom.
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∙ 13y ago
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∙ 15y agoThe Atomic Mass of the uranium isotope 238 is: 238,050 788 247 ± 0,000 002 044 atomic unit of mass.
Wiki User
∙ 7y agoThe atomic weight (not molar mass) of uranium-238 is 238,050 788 247 ± 0,000 002 044 u.
Wiki User
∙ 14y agothere are (238-92)= 146 neutrons
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∙ 11y ago238
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What does 238 represent in uranium?
Uranium-238 is a natural isotope of uranium with the mass 238,050 788 247 ± 0,000 002 044 u.a.
What element has the atomic number 238?
There is NO element with the Atomic No. of 238. Atomic No. only go to ~ 110. However, There is an element with ATOMIC MASS of 238, it is an isotope of Uranium NB . Atomic Number refers to #1 the position in the periodic table #2 the number of protons in the element #3 the number of electrons in the neutrally charged element. Atmoic Mass refers to the Sum total of all the protons and neutrons in the nucleus of an element. An element such as Uranium would be shown in the periodic table as [238/92]U. The two numbers indicating the Atomic Mass and the Atomic Number.
How many neutrons are stuffed into the nucleus of uranium-238?
Uranium-238 has 146 neutrons.
In Uranium-238 and Uranium-234 does neither element have a charge?
Uranium-238 and uranium-234 are not "elements", but they are natural isotopes of the chemical element uranium. The atoms are neutral.
What are the similarities and differences between the isotopes uranium 235 and uranium 238?
Uranium-235 has 143 neutrons and uranium-238 has 146 neutrons. And of course the atomic masses are different.
What are the molar masses of uranium 238 and uranium 235?
U-238 and U-235 are the two isotopes of Uranium. Molar mass M is not the right expression for each isotope. The naturally occurring Uranium has the following composition : 0.7% U-235, its Atomic Mass is 235.043 amu (amu is atomic mass unit), and. 99.3% U-238, its atomic mass is 238.05 amu.
What are the molar mass of uranium 238?
Pure Uranium-238 has an Atomic Mass of 238.1252 amu. Thus one mole of it weighs 238.1252 grams.
What are the molar masses of uranium -238 and uranium -235?
U-238 and U-235 are the two isotopes of Uranium. Molar mass M is not the right expression for each isotope. The naturally occurring Uranium has the following composition : 0.7% U-235, its atomic mass is 235.043 amu (amu is atomic mass unit), and. 99.3% U-238, its atomic mass is 238.05 amu.
What is the molar mass of one mole of Uranium?
1 atomgram of uranium = 238,02891 gramsAnswer:The molar mass of Uranium is 238.03 g/mol
What is the mass number of urnanium?
Uranium is a non metal element. Atomic mass of it is 238.
What do the '238' in uranium-238 and the '14' in carbon-14 mean?
* 238 is the atomic mass of a natural uranium isotope. * 14 is the atomic mass of a carbon isotope.
What does 238 represent in uranium?
Uranium-238 is a natural isotope of uranium with the mass 238,050 788 247 ± 0,000 002 044 u.a.
Uranium-235 and uranium-238 are different?
Uranium-235 and uranium-238 are different isotopes of the element uranium. They have different mass numbers due to different numbers of neutrons.
What is the molar mass of uranium in nuclear reactors?
The atomic weight of uranium is 238,02891.
What is the mass of uranium-238?
The atomic mass of the isotope uranium-238 is 238,050 788 247 ± 0,000 002 044 (Audi, Wapstra & Thibault-2003).
What is the weight of uranium?
Atomic mass number = Number of protons + Number of neutrons Number of protons of uranium nucleus is 92. The number of neutrons is different for each isotope. Example for 238U: 92 protons + 146 neutrons = 238
The atomic number of uranium is 92 and its atomic mass is 238.how many neutrons does the most common isotope of uranium have.?
The most common isotope of uranium is uranium-238 with 146 neutrons.
