Question

One of the wavelengths of light emitted by hydrogen atoms is 6.56 x 10-7 m. Calculate the Energy.

Answer 1

The Energy of an atom of hydrogen with wavelength 6.56 × 10⁻⁷ m is
 3.028 × 10⁻¹⁹ J.

I attached the working out and the answer to the question below.

Please note that C = speed of light, ν = frequency, λ= wavelength, h = Planck's Constant

Answer 2

The energy given wavelengths of light emitted by hydrogen atoms is 3.028 × 10⁻¹⁹ J.

The energy of the wavelength can be calculated by the  

$\bold {E = h \dfrac c\lambda}$

Where,  

C = speed of light,

ν = frequency,

λ= wavelength,

h = Planck's Constant

put the values in the formula,

$\bold {E = 6.626x10^{-34} \ J.s( \dfrac {2.998x 10^8\\\\ m/s}{6.56x 10^{-7}})}\\\bold {E = 3.028x10^{-19}J}$

Therefore,  the energy given wavelengths of light emitted by hydrogen atoms is 3.028 × 10⁻¹⁹ J.

To know more about wavelength,

https://brainly.com/question/7143261