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sineoko [7]
3 years ago
14

The photoionization of N2 in the thermosphere absorbs much of the high-energy radiation coming from the sun. If the ionization e

nergy of N2 is 1495 kJ/mol, what is the maximum wavelength of a photon that would have sufficient energy to ionize N2? To which region of the electromagnetic spectrum does this photon belong?
Chemistry
1 answer:
muminat3 years ago
3 0

Answer:

1.33 × 10⁻³¹ m

Gamma rays

Explanation:

1 mol of photons required for the photoionization of N₂ has an energy (E) of 1495 kJ = 1495 × 10³ J = 1.495 × 10⁶ J. We can find the wavelength (λ) associated with this energy using the Planck-Einstein equation.

E = h . c . λ⁻¹

where,

h is the Planck's constant

c is the speed of light

E = h . c . λ⁻¹

λ = h . c . E⁻¹ = (6.63 × 10⁻³⁴ J.s) . (3.00 × 10⁸ m/s) . (1.495 × 10⁶ J)⁻¹ = 1.33 × 10⁻³¹ m

This wavelength corresponds to the Gamma rays region of the spectrum.

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Hey there!

325 mL in liters:

325 / 1000 => 0.325 L

1 mole ( Ne ) ------------- 22.4 L ( at STP )

moles ( Ne ) ------------ 0.325 L

moles Ne = 0.325 * 1 / 22.4

moles Ne = 0.325 / 22.4

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hope this helps!

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