Calculate the energy required for the process.
He⁺(g) → He²⁺(g) + e⁻
The ionisation energy for the H atom in its ground state is - 13.6 ev atom⁻¹.
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Given conditions ⇒
Ionization Energy = -13.6 eV atom
= 13.6 × 1.6 × 10⁻¹⁹ J/atom.
= 2.176 × 10⁻¹⁸ J/atom.
We know that He ion is single electron species which resembles the Hydrogen.
Now, Using the Expressions which gives the energies of the stationary orbits of the Hydrogen like ions.
∴ Energy required = (I.E. )Z²/n²
Where,
Z = 2 and
n = 1 atom.
∴ E = (2.176 × 10⁻¹⁸)(2)²/(1)²
= 8704 × 10⁻¹⁸ J
Hope it helps.
Ionization Energy = -13.6 eV atom
= 13.6 × 1.6 × 10⁻¹⁹ J/atom.
= 2.176 × 10⁻¹⁸ J/atom.
We know that He ion is single electron species which resembles the Hydrogen.
Now, Using the Expressions which gives the energies of the stationary orbits of the Hydrogen like ions.
∴ Energy required = (I.E. )Z²/n²
Where,
Z = 2 and
n = 1 atom.
∴ E = (2.176 × 10⁻¹⁸)(2)²/(1)²
= 8704 × 10⁻¹⁸ J
Hope it helps.
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