Question 3 : Calculate the wavelength in angstroms of electromagnetic radiation emitted by a hydrogen atom which undergoes a transition between energy levels of -1.36×10−19J and ‘-5.45 ×10−19J. (Take Planck??s constant h = 6.6 ×10′−34Js)
E1– E2 = hf = hc/λ
E1 = -1.36×10−19J
E2 = 5.45 ×10−19J
- 6.6 ×10′−34Js
λ = ?
Solution
E1– E2 = hf = hc/λ
E don’t have frequency so we going to solve for frequency first
Frequency can be calculated using the following equation
E2 – E1 = hf
F = E2 – E1
h
-5.45 ×10−19J + 1.36×10−19J = 6.6 ×10′−34JsF making F the subject of the formula we have
F = -5.45 ×10−19J + 1.36×10−19J = -619696969696969.69696969696969697 approximately is
6.6 ×10′−34Js
= 6.2 X 1015Hz
F = 6.2 X 1015Hz
Now we want to look for wavelength
Which is E1– E2 = hc/λ
Λ = hc/ E1– E2
So we
E1 = -1.8eV
E2 = -4.0eV
-1.8 + 4.0 = 2.2ev
H = 6.6 ×10′−34Js
C = 3 .0 ×10′8ms-1
6.6 ×10′−34Js x 3 .0 ×10′8ms-1 = 0.000000000000000000000000198
Λ = —————————————————————————————————– =
2.2 x 3 .0 ×10′8ms-1 = 0.000000000000000352
=0.0000000005625 approximately = 5.625 x 3 .0 ×10′-10m answer
The post Question 3 : Calculate the wavelength in angstroms of electromagnetic radiation emitted by a hydrogen atom which undergoes a transition between energy levels of -1.36×10−19J and ‘-5.45 ×10−19J. (Take Planck??s constant h = 6.6 ×10′−34Js) appeared first on Omokosaban.com.
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