Question

The teal line of the hydrogen emission spectrum has a wavelength of 486.0 nm. A hydrogen emission spectrum has a violet, a blue, a teal, and a red line. Calculate the energy of one photon of this light.

Answer 1

Answer:

The correct answer to the following question will be "4.08 × 10⁻¹⁹ Joule".

Explanation:

Given:

Wavelength, λ = 486.0 nm

As we know,

$E=h\upsilon =\frac{hc}{\lambda}$

On putting the estimated values, we get

⇒          $=\frac{1241.5 \ ev\ nm}{486 \ nm}$

⇒          $=2.554 \ ev$

∴ 1 ev = 1.6 × 10⁻¹⁹ J

Now,

Energy, $E=2.554\times 1.6\times 10^{-19}$

⇒               $=4.08\times 10^{-19} Joule$