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Question
Energy of an electron in the ground state of the hydrogen atom is –2.18 × 10–18 J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol–1.
Energy of an electron in the ground state of the hydrogen atom is –2.18 × 10–18 J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol–1.
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Solution
The energy of an electron in the ground state of the hydrogen atom is –2.18 × 10–18 J. Therefore, the energy required to remove that electron from the ground state of hydrogen atom is 2.18 × 10–18 J.
∴ Ionization enthalpy of atomic hydrogen = 2.18 × 10–18 J
Hence, ionization enthalpy of atomic hydrogen in terms of J mol–1
= 2.18 × 10–18 × 6.02 × 1023 J mol–1 = 1.31 × 106Jmol–1
The energy of an electron in the ground state of the hydrogen atom is –2.18 × 10–18 J. Therefore, the energy required to remove that electron from the ground state of hydrogen atom is 2.18 × 10–18 J.
∴ Ionization enthalpy of atomic hydrogen = 2.18 × 10–18 J
Hence, ionization enthalpy of atomic hydrogen in terms of J mol–1
= 2.18 × 10–18 × 6.02 × 1023 J mol–1 = 1.31 × 106Jmol–1
Suggest Corrections
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