Chem homework help?
2016-06-24 1:29 pm
Carbon dioxide in the atmosphere acts as a greenhouse gas by absorbing infrared radiation at a wavelength of 15um. What is the frequency? What is the energy of a single photon of this emission (J)? What is the energy of a mole of photons at this wavelength (J/mole)?
回答 (1)
2016-06-24 2:03 pm
Speed of light, c = 3 × 10⁸ m/s
Planck constant, h = 6.626 × 10⁻³⁴ J s
Avogadro constant, N = 6.022 × 10²³ /mol
Frequency, ν
= c/λ
= (3 × 10⁸) / (15 × 10⁻⁶) Hz
= 2 × 10¹³ Hz
Energy of a single proton
= hν
= (6.626 × 10⁻³⁴) × (2 × 10¹³) J
= 1.33 × 10⁻²⁰ J
Energy of a mole of photon at this wavelength
= Nhν
= (6.022 × 10²³) ×(6.626 × 10⁻³⁴) × (2 × 10¹³) J/mol
= 7980 J/mol
Planck constant, h = 6.626 × 10⁻³⁴ J s
Avogadro constant, N = 6.022 × 10²³ /mol
Frequency, ν
= c/λ
= (3 × 10⁸) / (15 × 10⁻⁶) Hz
= 2 × 10¹³ Hz
Energy of a single proton
= hν
= (6.626 × 10⁻³⁴) × (2 × 10¹³) J
= 1.33 × 10⁻²⁰ J
Energy of a mole of photon at this wavelength
= Nhν
= (6.022 × 10²³) ×(6.626 × 10⁻³⁴) × (2 × 10¹³) J/mol
= 7980 J/mol
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