Browse by Stream
QnA
Home
QnA
Go To Your Study Dashboard

Get Answers to all your Questions

header-bg qa
  • Home
  • NCERT
  • Energy of an electron in the ground state of the hydrogen atom is minus 2.18×10 raised to minus 18J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol raised to minus 1.

3.15   Energy of an electron in the ground state of the hydrogen atom is -2.18 \times 10 ^{-18 }J  Calculate the ionization enthalpy of atomic hydrogen in terms of  J mol ^{-1}

Answers (1)

best_answer

Given that Energy of an electron in the ground state of the hydrogen atom is -2.18 \times 10 ^{-18 }J.

So, the ionization enthalpy is for 1 mole of atoms.

Therefore, the ground state energy of the atoms may be expressed as :

E (ground state) = -2.18 \times 10 ^{-18 }J \times (6.022\times 10^{23} mol^{-1})

= -1.312\times 10^{6} J\ mol^{-1}

Whereas, ionization enthalpy is, 

=E_{\infty } - E_{ground\ state}

=0-(-1.312\times10^6 mol^{-1}) =1.312\times10^{6} J\ mol^{-1}

Posted by

Divya Prakash Singh

View full answer

Crack CUET with india's "Best Teachers"

  • HD Video Lectures
  • Unlimited Mock Tests
  • Faculty Support
cuet_ads

Similar Questions

Trending Articles/News

anam-khan

CBSE Class 12 board exams 2025 to have 50% competency-based questions; no change in 10th
anam-khan

CBSE Class 12 board exams 2024 over; expected result date, trends of last 10 years
anam-khan

CBSE Class 12 accountancy board exam analysis 2024 out; paper rated easy, balanced

Latest Question