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Luba_88 [7]
2 years ago
15

An Argon laser gives off pulses of green light (wavelength = 514 nm). If a single pulse from the laser has a total energy of 10.

0 mJ how many photons are in the pulse?
Chemistry
1 answer:
svetoff [14.1K]2 years ago
7 0

Answer:

n=2.59\times 10^{16} photons

Explanation:

E=n\times \frac{h\times c}{\lambda}

Where,  

n is the number of photons

h is Plank's constant having value 6.626\times 10^{-34}\ Js

c is the speed of light having value 3\times 10^8\ m/s

\lambda is the wavelength of the light

Given that, wavelength = 514 nm = 514\times 10^{-9}\ m

Energy = 10.0 mJ = 0.01 J ( 1 mJ = 0.001 J )

Applying the values as:-

0.01=n\times \frac{6.626\times 10^{-34}\times 3\times 10^8}{514\times 10^{-9}}

\frac{19.878n}{10^{17}\times \:514}=0.01

n=2.59\times 10^{16} photons

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<u>Answer:</u> The percentage abundance of _{17}^{35}\textrm{Cl} and _{17}^{37}\textrm{Cl} isotopes are 75.77% and 24.23% respectively.

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\text{Average atomic mass }=\sum_{i=1}^n\text{(Atomic mass of an isotopes)}_i\times \text{(Fractional abundance})_i   .....(1)

Let the fractional abundance of _{17}^{35}\textrm{Cl} isotope be 'x'. So, fractional abundance of _{17}^{37}\textrm{Cl} isotope will be '1 - x'

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Fractional abundance of _{17}^{35}\textrm{Cl} isotope = x

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Percentage abundance of _{17}^{35}\textrm{Cl} isotope = 0.7577\times 100=75.77\%

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Hence, the percentage abundance of _{17}^{35}\textrm{Cl} and _{17}^{37}\textrm{Cl} isotopes are 75.77% and 24.23% respectively.

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