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german
3 years ago
14

An intense emission line for a new element is observed at a wavelength of 675 nm. What is the energy of a single photon of this

light?Energy = ___.
Chemistry
1 answer:
andreyandreev [35.5K]3 years ago
7 0

Answer:

E=2.95\times 10^{-19}\ J

Explanation:

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

Where,  

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, \lambda=675\ nm=675\times 10^{-9}\ m

Thus, applying values as:

E=\frac{6.626\times 10^{-34}\times 3\times 10^8}{675\times 10^{-9}}\ J

E=\frac{10^{-26}\times \:19.878}{10^{-9}\times \:675}\ J

E=2.95\times 10^{-19}\ J

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First step is to calculate the mass of Ag in each compound separately:
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For AgCl, mass % of Ag = [107.87/143.32] x 100 = 75.26%
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Second step is to calculate the mass % of each compound in the mixture:
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