The wavelength of a photon that has energy of 1j is 19.878 ×10^-17 nm.
The energy of photon is given by,
E=h × frequency
where h is known as planck's constant whose value is
[tex]6.626 \times {10}^{ - 34} js[/tex]
Frequency : it is the reciprocal of time period . it can be defined as number of Occurance of repeating events per unit time.
f=1/T
si unit is :
[tex] {s}^{ - 1} [/tex]
The formula of frequency is :
f = c/ lambda
where c is the velocity of light whose value is 3×10^8m/s and lambda is the wavelength.
Thus,
[tex]energy = \frac{h.c}{lambda} [/tex]
And,
[tex]wavelength = \frac{h.c}{energy} [/tex]
[tex]lambda = \frac{6.626 \times {10}^{ - 34} js \times 3 \times {10}^{8} \frac{m}{s} }{1j } = 19.878 \times {10}^{ - 26} m[/tex]
Hence the wavelength of photon is 19.878×10^-26 m Or 19.878×10^-17 nm.
Learn more about wavelength here:
brainly.com/question/10728818
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Disclaimer :the data in the question is incomplete that is the options are not correct or incomplete.
Question: what is the wavelength of a photon that has an energy of 1 j.
(a) 19.878×10^-17 nm
(b) 19.878×10^-18nm
(c) 19.878×10^-16nm
(d) 19.878×10^-15nm
(e) 19.878×10^-20nm
