## Related questions with answers

Molybdenum metal must absorb radiation with a minimum frequency of

$1.09 \times 10 ^ { 15 } \mathrm { s } ^ { - 1 }$

before it can eject an electron from its surface via the photoelectric effect. What wavelength of radiation will provide a photon of this energy?

Solutions

VerifiedTo calculate the wavelenght of the radiation we will use the expression:

$c=\lambda \cdot \nu$

where $\lambda$, $\nu$ is the wavelength, $\nu$ is the frequency and c is the speed of light which is a constant. When we insert the values of c and $\nu$ we get:

$\lambda=\frac{c}{\nu}=\frac{3\cdot10^8}{1.09\cdot10^{15}}=275 \cdot10^{-9} \text{m}=275 \text{nm}$

$\lambda=\dfrac{c}{v}$

$=\dfrac{3.0\times10^{8}\dfrac{m}{s}}{1.09\times10^{15}s^{-1}}$

$=2.75\times10^{-7}m$

$=275\times10^{-9}m$

Calculate the wavelength

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