Two atoms interact with each other and change as shown by the equation. complete the equation by filling in the missing parts.

the missing parts are ³₂He

Explanation:

The equation shown represents a nuclear reaction, meaning that, instead of the two hydrogen atoms form a molecule by a chemcial bond between the electrons of the atoms, the nuclei of the two interacting atoms change, leading to a new kind of atoms and particles.

That is mainly indicated by the appearace of the particle ¹₀ n, which is the symbol for a neutron.  The superscript 1 to the left of the symbol (letter n) means that the mass number of the neutron is 1, and the subscript 0 to the left of the symbol means that the atomic number of neutron is 0.

To determine the symbol, superscript and subscript needed to complete the missing parts of the equation, you need to do a mass number and atomic number balance.

Mass number balance:

The mass number is the superscript to the left of the symbol of the atom.

Each hydrgogen atom, in the reactant side, contributes a mass number 2, and the neutron on the product side contributes a mass number 1, so the balance is:

    2 + 2 = x + 1,

from which you determine that the unknown mass number is x = 4 - 1 = 3.

Atomic number balance

The atomic number is the subscript to the left of the element.

Each hdyrogen atom contributes an atomic number 1, and the neutron contributes 0 atomic number. So, the atomic number balance is:

    1 + 1 = x + 0 ⇒ x = 2.

Hence, the unknown atomic number is 2.

Conclusions:

         ²₁ H + ²₁ H  → ³₂He + ¹₀ p

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.