Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: Rutherford on August 30, 2012, 01:54:42 PM
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The formula is:
E=(mi-mf)c2
mi=initial mass, mf=final mass
I only found problems where those masses are expressed in unified atomic mass unit, this should be applied only for one atom, but when I have, for example, 100kg of uranium 239 and by beta decay it decays to 239Np, let's say 50kg was made, how to calculate the energy released?
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The formula is:
E=(mi-mf)c2
mi=initial mass, mf=final mass
I only found problems where those masses are expressed in unified atomic mass unit, this should be applied only for one atom, but when I have, for example, 100kg of uranium 239 and by beta decay it decays to 239Np, let's say 50kg was made, how to calculate the energy released?
What is the exact mass of 239U?
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The atomic mass of uranium is 239.05429.
Of neptunium 239.05293.
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I think no needed. If from 100 Kg U 50 kg converted to Np then 50 kg has to be left
E = 50 kg * (300.000.000 m/s)2 = 4,5 x 1018 J
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I think no needed. If from 100 Kg U 50 kg converted to Np then 50 kg has to be left
E = 50 kg * (300.000.000 m/s)2 = 4,5 x 1018 J
Possibly, given the sig fig issues, yes. But does 50 kg exactly of 239U yield 50 kg exactly of 239Np ?
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Possibly, given the sig fig issues, yes. But does 50 kg exactly of 239U yield 50 kg exactly of 239Np ?
Probably not. But compared will be E=(mi-mf)c2
mi=initial mass, mf=final mass
So it doesn't matter what is the yield.
The mass difference of a neutron and a proton is the difference. In U 239 one Neutron will be converted to a Proton to get Np 239.
50 Kg U means 49.999972 kg Np
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I tried another way. I used first the unified atomic masses converted to kg, and I got that E=2.04*10-13J, this is the energy released when 1 atom of uranium gets decayed. In the example (50000/239)*6*1023=1.255*1026 atoms decayed. So the energy released is E*N=2.56*1013J. Why our results difference so much?
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How do you calculate E = 2.04* 10-13 J?
U MG = 239 g/mol contain 92 Protones and 147 Neutrons
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Mass difference is 239.05429u-239.05293u=0.00136u=2.2583*10-30kg, so E=2.0325*10-13J (small difference because I used numbers with more digits now).
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No that is not the mass. You calculated the mass defect.
The mass is 92 x mass of proton + 147 x mass of neutron = mass of 1 atom.
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But the mass defect is caused by the released energy.
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The question is 50 kg Uranium disappeared and 50 kg or a little bit less Neptunium is created.
23992U => 23993Np + ß
I am wrong you are right its the mass of the defect to be taken.
http://en.wikipedia.org/wiki/Decay_energy
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Okay, I got confused because I read some text about the mass defect. 50kg of Np was made so a little more than 50kg of U decayed (because mass of n0 is bigger than the mass of p+), now I use that mass as Δm to calculate the energy released.
Where does the released energy then come from?
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http://www.science.uwaterloo.ca/~cchieh/cact/nuctek/decayenergy.html
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Then it should be: Δm=the mass that decayed(not 100kg) - the mass of Np.
Δm=2.8446*10-4g
E=2.56*10-13J again.
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correct