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Class 11
Chemistry
Classification of Elements and Periodicity in Properties
energy of an electron in the ground state of the h...

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.

Answer:

Ionization enthalpy is the minimum amount of energy which is needed to remove the loosely bound electron from a 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.

Therefore, the energy required to remove that electron from the ground state of hydrogen atom is 2.18 × 10^–18J.

so Ionization enthalpy of atomic hydrogen = 2.18 × 10^–18J

Hence, ionization enthalpy of atomic hydrogen in terms of J mol^–1 = 2.18 × 10^–18 × 6.02 × 10²³ J mol^–1 = 1.31 × 10⁶ J mol^–1

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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.

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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.

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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.