Answer:
A
Explanation:
The energy E of a photon is
directly proportional to its frequency f by E = hf, where h is Planck's constant (above)
and the wavelength w is inversely proportional to the frequency by w = c/f, so we have
E related to w by: E = hc/w. Since h and c are constants, their product hc is constant
being 1.989 * 10**-25 joule-meters. So if we know E is 1.32 * 10**-18 J, we have:
1.32 * 10**-18 = (1.989 * 10**-25) / w or w = (1.989 * 10**-25) / (1.32 * 10**-18) Doing
the division and we find w = 1.507 x 10-7 meters, or 150.7 nanometers. (ultraviolet)
A. 150 x 10-7nm
We have that when the energy of a photon is 1.32 × 10¯18 j, what is its wavelength in nm
[tex]\lambda=150nm[/tex]
From the question we are told that
energy of a photon is 1.32 × 10¯18 j
Generally the equation for the energy of a photon is mathematically given as
[tex]e=\frac{hc}{\lamda}\\\\1.32 x 10{-18}=\frac{6.6*10^-34*3*10^8}{\lamda}\\\\\lambda=15.04*10^{-8}[/tex]
[tex]\lambda=150nm[/tex]
Therefore
When the energy of a photon is 1.32 × 10¯18 j, what is its wavelength in nm
[tex]\lambda=150nm[/tex]
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