Question

Wavelength for high energy EMR transition in H-atom is 91 nm. What energy is needed for this
transition?
(a) 1.36 eV
(b) 1240 eV
(c) 13 eV
(d) 13.6 eV​

Answer 1

Answer:

Step-by-step explanation:

wavelength (λ)  = 91nm;

We know that Energy = hv = hcλ

h is planck constant and c is the velocity of light

By putting the value of those constant we will calculate the answer

E = 6.626*10^-34 * 3*10^8*91*10^-9

E = 0.2184*10^-17 J;

now converting into eV;

E = 136 eV

Answer 2

Given that,

Wavelength for high energy EMR transition in H-atom is 91 nm.

To find,

The energy needed for this transition

Solution,

The energy needed is given in terms of its wavelength by the below formula as :

$E=\dfrac{hc}{\lambda}$

h is plank's constant and c is speed of light

So,

$E=\dfrac{6.63\times 10^{-34}\times 3\times 10^8}{91\times 10^{-9}}\\E=2.18\times 10^{-18}\ J$

We know that,

$1\ eV=1.6\times 10^{-19}\ J$

$E=\dfrac{2.18\times 10^{-18}}{1.6\times 10^{-19}}\\E=13.6\ eV$

So, 13.6 eV of energy is needed for this  transition.

Learn more,

Wavelength for high energy EMR transition in H-atom is 91 nm. What energy is needed for this  transition?

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