Problem Page
It takes
163./kJmol
to break an nitrogen-nitrogen single bond. Calculate the maximum wavelength of light for which an nitrogen-nitrogen single bond could be broken by absorbing a single photon.
Round your answer to
3
significant digits.
Maximum wavelength Please help?
2016-10-02 4:51 am
回答 (1)
2016-10-02 5:03 am
Avogadro constant = 6.023 × 10²³ /mol
Planck constant, h = 6.626 × 10⁻³⁴ J s
Speed of light, c = 3.00 × 10⁸ m/s
Energy, E = 157 kJ/mol = 157 × 10³ J/mol
E = N h ν and ν = c / λ
Hence, E = N h c / λ
λ = N h c / E
Maximum wavelength, λ
= N h c / E
= (6.023 × 10²³ /mol) × (6.626 × 10⁻³⁴ J s) × (3.00 × 10⁸ m/s) / (157 × 10³ J/mol)
= 7.63 × 10⁻⁷ m
= 763 × 10⁻⁹ m
= 763 nm
Planck constant, h = 6.626 × 10⁻³⁴ J s
Speed of light, c = 3.00 × 10⁸ m/s
Energy, E = 157 kJ/mol = 157 × 10³ J/mol
E = N h ν and ν = c / λ
Hence, E = N h c / λ
λ = N h c / E
Maximum wavelength, λ
= N h c / E
= (6.023 × 10²³ /mol) × (6.626 × 10⁻³⁴ J s) × (3.00 × 10⁸ m/s) / (157 × 10³ J/mol)
= 7.63 × 10⁻⁷ m
= 763 × 10⁻⁹ m
= 763 nm
收錄日期: 2021-04-18 15:36:34
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