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Misteh
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I have just started AP Chemistry this year as a junior at my high school despite all peer protests against it. And I admit so far the course has lived up to it's reputation of being very difficult. I was rather ecstatic to come across this site where I may obtain the help I /know/ I will need all year. So expect to see me often. ^_^
We use the 7th edition Chemistry textbook by Zumdahl, so I believe my source is familiar to at least some.
Calculate the energy released per (4 mass #, 2 Protons)He nucleus produced and per moles of (4 mass #, 2 Protons)He produced. The atomic masses are (2,1)H, 2.01410; (3,1)H, 3.01605; and (4,2)He, 4.00260. The masses of the electron and neutron are 5.4858 x 10 raised to the -4 and 1.00866 amu, respectively.
The easiest fusion reaction to initiate is
(2,1) H + (3,1) H ---> (4,2) He + (0,1) n
∆m = (4.00260 + 1.00866) - (2.01410 + 3.01605) = -1.02755 amu
(Originally I had the two enclosed equations swapped which would give a positive result instead. Would this matter? If so, why?)
For Mole;
-1.02755 amu = 1.6005 x 10 to the -27 Kg / 1 amu
= -1.6446 Kg
E= mc squared, so: -1.6446 Kg x (2.997 x 10 to the 8) Squared
= 49289 J
For Nucleus;
I was unsure how to find this, but I found that
1 mol = 6.0221 x 10 to the 23 nuclei
So do I need to convert Kg into mol and then into nuclei?
We use the 7th edition Chemistry textbook by Zumdahl, so I believe my source is familiar to at least some.
Homework Statement
Calculate the energy released per (4 mass #, 2 Protons)He nucleus produced and per moles of (4 mass #, 2 Protons)He produced. The atomic masses are (2,1)H, 2.01410; (3,1)H, 3.01605; and (4,2)He, 4.00260. The masses of the electron and neutron are 5.4858 x 10 raised to the -4 and 1.00866 amu, respectively.
Homework Equations
The easiest fusion reaction to initiate is
(2,1) H + (3,1) H ---> (4,2) He + (0,1) n
The Attempt at a Solution
∆m = (4.00260 + 1.00866) - (2.01410 + 3.01605) = -1.02755 amu
(Originally I had the two enclosed equations swapped which would give a positive result instead. Would this matter? If so, why?)
For Mole;
-1.02755 amu = 1.6005 x 10 to the -27 Kg / 1 amu
= -1.6446 Kg
E= mc squared, so: -1.6446 Kg x (2.997 x 10 to the 8) Squared
= 49289 J
For Nucleus;
I was unsure how to find this, but I found that
1 mol = 6.0221 x 10 to the 23 nuclei
So do I need to convert Kg into mol and then into nuclei?