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LekaFEV [45]
3 years ago
12

A hydrogen atom requires a minimum energy of 2.18×10^-18 J atom to remove an electron from its ground state level. Determine whe

ther a blueviolet light with a wavelength of 434.0 nm can affect this process.
Chemistry
1 answer:
frosja888 [35]3 years ago
5 0
Just find the energy of the <span>blueviolet light with a wavelength of 434.0 nm using the formula:

E  = hc / lambda

E = energy
c= speed of light =  3 x 10^8 m/s
h = planck's constant =  6.6 x 10^{-34}  m^2 kg / s
lambda =  434 nm =  434 x 10^{-9} m

Putting these values (with appropriate units) in the above formula :

we get:  Energy, E = 4.5 x 10^{-19} J

E = 0.45 x 10^{-18} J

Now, the </span>minimum energy is 2.18×10^-{18} J but our energy is 0.45 x 10^{-18} J which is less.
<span>Means the electron will not be removed

</span>
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An 80.0g sample of an unknown metal is at an initial temperature of 55.5oC. Afer 540 J of energy is absorbed by the metal, the t
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Q = m.c. ΔT

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