The energy required by electrons, present in the first Bohr orbit of hydrogen atom to be excited to the second Bohr orbit is ______

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Q.
The energy required by electrons, present in the first Bohr orbit of hydrogen atom to be excited to the second Bohr orbit is _______ $J {mol}^{- 1}$ .

Given: $R_{H} = 2.18 \times 10^{- 11} ergs$ [2026]

1 $9.835 \times 10^{12}$

2 $9.835 \times 10^{5}$

3 $1.635 \times 10^{- 11}$

4 $1.635 \times 10^{- 18}$

Ans.
(2)

$E_{n} = - R_{H} \times \frac{Z^{2}}{n^{2}}$

$Δ E = 2.18 \times 10^{- 11} \times 10^{- 7} \times 1^{2} [\frac{1}{1^{2}} - \frac{1}{2^{2}}]$

$= 1.635 \times 10^{- 18} Joule/atom$

$= 1.635 \times 10^{- 18} \times 6.02 \times 10^{23} Joule/mole$

$= 9.835 \times 10^{5} Joule/mole$

Solution

Q.
The energy required by electrons, present in the first Bohr orbit of hydrogen atom to be excited to the second Bohr orbit is _______ $J {mol}^{- 1}$ .

Given: $R_{H} = 2.18 \times 10^{- 11} ergs$ [2026]

1 $9.835 \times 10^{12}$

2 $9.835 \times 10^{5}$

3 $1.635 \times 10^{- 11}$

4 $1.635 \times 10^{- 18}$

Ans.
(2)

$E_{n} = - R_{H} \times \frac{Z^{2}}{n^{2}}$

$Δ E = 2.18 \times 10^{- 11} \times 10^{- 7} \times 1^{2} [\frac{1}{1^{2}} - \frac{1}{2^{2}}]$

$= 1.635 \times 10^{- 18} Joule/atom$

$= 1.635 \times 10^{- 18} \times 6.02 \times 10^{23} Joule/mole$

$= 9.835 \times 10^{5} Joule/mole$

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Solution

Q. The energy required by electrons, present in the first Bohr orbit of hydrogen atom to be excited to the second Bohr orbit is _______ J mol-1. Given: RH=2.18×10-11 ergs [2026]

1 9.835×1012

2 9.835×105

3 1.635×10-11

4 1.635×10-18

Ans. (2) En=-RH×Z2n2 ΔE=2.18×10-11×10-7×12[112-122] =1.635×10-18 Joule/atom =1.635×10-18×6.02×1023 Joule/mole =9.835×105 Joule/mole

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Q.
The energy required by electrons, present in the first Bohr orbit of hydrogen atom to be excited to the second Bohr orbit is _______ $J {mol}^{- 1}$ .

Given: $R_{H} = 2.18 \times 10^{- 11} ergs$ [2026]

1 $9.835 \times 10^{12}$

2 $9.835 \times 10^{5}$

3 $1.635 \times 10^{- 11}$

4 $1.635 \times 10^{- 18}$

Ans.
(2)

$E_{n} = - R_{H} \times \frac{Z^{2}}{n^{2}}$

$Δ E = 2.18 \times 10^{- 11} \times 10^{- 7} \times 1^{2} [\frac{1}{1^{2}} - \frac{1}{2^{2}}]$

$= 1.635 \times 10^{- 18} Joule/atom$

$= 1.635 \times 10^{- 18} \times 6.02 \times 10^{23} Joule/mole$

$= 9.835 \times 10^{5} Joule/mole$