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15/08/2021 11:30 am
Topic starter
Based on the equation:
▵E = -2.0 x 10-18J (\(\frac{1}{n_2^2}- \frac{1}{n_1^2}\))
the wavelength of the light that must be absorbed to excite hydrogen electron from level n = 1 to level n = 2 will be:
(h = 6.625 × 10-34 Js, C = 3 × 108 ms-1)
(a) 1.325 × 10-7 m
(b) 1.325 × 10-10 m
(c) 2.650 × 10-7 m
(d) 5.300 × 10-10 m
1 Answer
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15/08/2021 11:36 am
Correct answer: (a) 1.325 × 10-7 m
Explanation:
▵E = -2.0 x 10-18J (\(\frac{1}{n_2^2}- \frac{1}{n_1^2}\))
= -2.0 x 10-18 x \(\frac{-3}{4}\)
= 1.5 x 10-18
▵E = \(\frac{hc}{\lambda}\)
\(\lambda = \frac{hc}{\triangle E}\)
= \(\frac{6.6 \times 10^{-34} \times 3 \times 10^8}{1.5 \times 10^{-18}}\)
= 1.325 × 10-7 m