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  • According to Einstein's quantum theory, the energy of one quantum of light is given by <img alt="E=\frac{h c}{\lambda}" src="https://entrancecorner.oncodecogs.com/gif.latex?E%3D%5Cfrac%7Bh

According to Einstein's quantum theory, the energy of one quantum of light is given by E=\frac{h c}{\lambda}  where h is Planck's constant, c is the speed of light and  {\lambda} is the wavelength of light. What is the wavelength of a photon of light having an energy of 3.0 eV?

 

Option: 1

414 nm


Option: 2

480 nm


Option: 3

620 nm


Option: 4

700 nm


Answers (1)

best_answer

The energy of the photon is 3.0 eV.

We can convert this to joules using the conversion factor 1 eV=1.6\times10^{-19 }J . 

Therefore, the energy of the photon is 4.8\times10^{-19 }J 

Now, we can rearrange the formula to solve for {\lambda}, 

E=\frac{h c}{\lambda} 

Plugging in the values we have, we get  

\lambda=\frac{\left(6.626 \times 10^{-34} \mathrm{~J} \mathrm{~s}\right) \times\left(3.00 \times 10^8 \mathrm{~m} / \mathrm{s}\right)}{4.8 \times 10^{-19} \mathrm{~J}}=4.14 \times 10^{-7} \mathrm{~m} \text {. }

Converting this to nanometers, we get 414 nm.  

Posted by

Suraj Bhandari

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