Rubidium was named after the red color observed in a flame test based on its emission at 645.8 nm. What is the total energy released , in kilojoules, by this emission when 37.0g of rubidium is subjected to a flame test? Assume each rubidium atom emits one photon at 645.8 nm.
Energy released by one photon
E = h*c/wavelength
= 6.626*10^-34 * 3*10^8 / ( 645.8*10^-9)(in m)
= 3.08*10^-19 joules.
This energy is produced by 1 photon of 1 atom
Now moles of rubidium = mass / molar mass
= 37.0 / 85.5
= 0.4327 moles
1 moles have 6.022*10^23 atoms
0.4327 moles will have 6.022*10^23*0.4327
= 2.606*10^23 atoms
Total energy released by all the atoms
(2.606*10^23)*(3.08*10^-19)
= 80264.8 joules
Or 80.2648 kilojoules.
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