For the following fusion reaction, calculate the change in energy of the reaction in units of joules per mole.
2/1 H + 2/1H --> 3/1 H + 1/1 H
H-1 1.00782
H-2 2.0140
H-3 3.01603
H-4 4.00260
neutron 1.00866
The equation: (Change in E) = (c^2) (change in m)
c = the speed of light, 3x10^8 m/s
(change in m) = (mass of products) - (mass of reactants) Kg
1 mol contains 6.03 x 10^23 particles, so 1 mol H-1 weighs
1.00782 x1.6605x10^-27x6.03x10^23kg
=1.00911152 x 10^-3 kg amu Avogadro N
2H-1 = twice the above > H-2 2.014x1.00782 x1.6605x10^-27 x 6.03 x 10^23=2.0X10^-3kg
Loss of mass = [2.01822304 - 2.0165]x10^-3kg
=1.7x10^-3kg
E = mc^2
=1.7x10^-6 x (3x10^8)2
=1.7x10^-6 x 9x10^16
=1.53x10^9 j/mole
Get Answers For Free
Most questions answered within 1 hours.