Energy of an electron in the ground state of the hydrogen atom is –2.18×10^–18J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol^–1.
Hint: Apply the idea of mole concept to derive the answer.

Question

Energy of an electron in the ground state of the hydrogen atom is –2.18×10^–18J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol^–1.
Hint: Apply the idea of mole concept to derive the answer.

Philoid · Accepted Answer

Ionization enthalpy is the minimal quantity of energy which is demanded to get rid of the most loosely bound electron from a neutral isolated gaseous atom to form a cation.

It is given that the energy of an electron in the ground state of the hydrogen atom is -2.18 × 10^-18J.

So, Ionization enthalpy of atomic hydrogen = 2.18 × 10^-18 J.

So, converting the ionization enthalpy from Joules to J/mole

= 2.18 × 10^-18 × 6.02 × 10²³ J mol^-1

= 1.31 × 10⁶ J mol^-1

Therefore, the ionization enthalpy of hydrogen atom is 1.31 × 10⁶ J mol^-1.

Energy of an electron in the ground state of the hydrogen atom is –2.18×10–18J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol–1.Hint: Apply the idea of mole concept to derive the answer.

Energy of an electron in the ground state of the hydrogen atom is –2.18×10^–18J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol^–1.
Hint: Apply the idea of mole concept to derive the answer.