Answer:
The wavelength of sunlight that can cause this bond breakage is 242 nm
Explanation:
The minimum energy of the sunlight that'll break Oxygen-oxygen bond must match 495 KJ/mol
But 1 mole of any molecule contains 6.02 × 10²³ molecules/mol
Each molecule of Oxygen will require (495 × 10³)/(6.02 × 10²³) = 8.22 × 10⁻¹⁹ J
E = hf
v = fλ
f = v/λ
f = frequency of the sunlight
λ = wavelength of the sunlight
v = speed of light = 3.0 × 10⁸ m/s
E = hv/λ
λ = hv/E
h = Planck's constant = 6.63 × 10⁻³⁴ J.s
λ = (6.63 × 10⁻³⁴)(3 × 10⁸)/(8.22 × 10⁻¹⁹)
λ = 2.42 × 10⁻⁷ m = 242 nm.
The answer is n= 6.
What is Balmer series?
The Balmer series is the portion of the emission spectrum of hydrogen that represents electron transitions from energy levels n > 2 to n = 2. These are four lines in the visible spectrum. They are also known as the Balmer lines. The four visible Balmer lines of hydrogen appear at 410 nm, 434 nm, 486 nm and 656 nm.
For the Balmer series, the final energy level is always n=2. So, the wavelengths 653.6, 486.1, 434.0, and 410.2 nm correspond to n=3, n=4, n=5, and n=6 respectively. Since the last wavelength, 410.2 nm, corresponds to n=6, the next wavelength should logically correspond to n=7.
To solve for the wavelength, calculate the individual energies, E2 and E7, using E=-hR/(n^2). Then, calculate the energy difference between E2 (which is the final) and E7 (which is the initial). Finally, use lamba=hc/E to get the wavelength.
To learn more about emission spectrum click on the link below:
brainly.com/question/24213957
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Then the force will also be doubled
