What is the energy in joules of the 656 nm spectral line of hydrogen?

Question

Quizplus · Accepted Answer

To determine the energy in joules of the 656 nm spectral line of hydrogen, we need to use the formula: E = hc/λ, where h is Planck's constant (6.626 x 10^-34 J*s), c is the speed of light (2.998 x 10^8 m/s), and λ is the wavelength in meters.

First, we need to convert the wavelength from nm to meters:

656 nm = 656 x 10^-9 m

Plugging in the values, we get:

E = (6.626 x 10^-34 J*s)(2.998 x 10^8 m/s)/(656 x 10^-9 m)

Simplifying the expression gives:

E = 3.03 x 10^-19 J

Therefore, the best choice is B, which matches this value.

What Is the Energy in Joules of the 656 Nm