a minimum energy of 389 kJ/mol is required to break one nitrogen-to-hydrogen bond in ammonia (NH3). What is the minimum frequency of radiation having the necessary energy to break this bond?
a)7.30x10^14 s^-1
b)1.81x10^15 s^-1
c)9.75x10^14 s^-1
d)1.09x10^15 s^-1
e)5.50x10^14 s^-1
i want to know how to solve this
Thank you !!!
What is the frequency of reaction having the necessary energy to break this bond?
2016-05-11 3:00 pm
回答 (1)
2016-05-11 4:43 pm
✔ 最佳答案
Planck constant, h = 6.62607 × 10⁻³⁴ J sFrequency, ν = ? /s
Avogadro constant, N = 6.022 × 10⁻²³ / mol
To break 1 mole of N-H bonds, 1 mole of photons are needed.
Hence, 1 mole of photons carries 389 kJ of energy.
Nhν = 389000 J/mol
ν = (389000 J) / (Nh)
Frequency, ν
= (389000 J/mol) / [(6.022 × 10⁻²³ J s) × (6.62607 × 10⁻³⁴ /mol)]
= 9.75 × 10¹⁴ /s
...... The answer is : c. 9.75 × 10¹⁴ /s
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