Question

The reaction that will probably power the first commercial fusion reactor is:3 0 H + 2 1 H image from custom entry tool4 2 He + 1 0 nHow much energy would be produced per mole of reaction?Masses of atoms:3 1 H = 3.01605 amu 4 2 He = 4.00260 amu2 1 H = 2.0140 amu 1 0 n = 1.008665 amuThe difference in masses is 0.018785 amuIn scientific notation, what is the energy in kJ/mol?

Answer 1

The energy produced per mole of the reaction 3 1 H + 2 1 H -> 4 2 He + 1 0 n is approximately 3 x 10^14 kJ/mol.

Step-by-step explanation:

The reaction described is: 3 1 H + 2 1 H => 4 2 He + 1 0 n. To determine the energy produced per mole of reaction, we need to calculate the difference in masses between the reactants and the products. The mass of 3 1 H is 3.01605 amu, the mass of 2 1 H is 2.0140 amu, the mass of 4 2 He is 4.00260 amu, and the mass of 1 0 n is 1.008665 amu. The difference in masses is 0.018785 amu.

To calculate the energy in kJ/mol, we need to convert the mass difference to kg by dividing by Avogadro's number and dividing by 1000 to convert from grams to kilograms. Finally, we multiply by the speed of light squared (c^2) to convert from mass to energy. The speed of light is approximately 3 x 10^8 m/s. The total energy is approximately 3 x 10^14 kJ/mol.

Answer 2

2.8087*10^-12 kJ per mole of reaction (2.8087*10^-12 kJ/mol).

Step-by-step explanation:

To calculate the energy produced, we need to write a balanced equation for the reaction and determine the change in the masses of the reactants and products. Afterward, we can use the energy equation to determine the energy produced. The balanced equation for the nuclear reaction is shown below:

³₁H + ²₁H ⇒⁴₂He + ¹₀n

The masses of atoms are ³₁H is 3.01605 amu, ²₁H is 2.0140 amu, ⁴₂He is 4.00260 amu, and ¹₀n is 1.008665 amu.

change in mass Δm = (3.01605+2.0140) - (4.00260+1.008665) = 0.0188 amu

Energy produced, E = m*C^2

C is the speed of light = 3*10^8 m/s and 1 amu = 1.66*10^-27 kg

Therefore:

E = 0.0188*1.66*10^-27 * (3*10^8)^2 = 2.8087*10^-12 kJ per mole of reaction.

Therefore, in scientific notation, the energy released is 2.8087*10^-12 kJ/mol