It requires 799 kJ of energy to break one mole of carbon-oxygen double bonds in carbon dioxide. What
Interpretation:
The energy required to rupture one mole of
Concept introduction:
Bohr developed a rule for quantization of energy that could be applicable to the electron of an atom in motion. By using this he derived a formula for energy levels of electron in H-atom.
Relation between frequency and wavelength is,
C is the speed of light.
h is Planck’s constant (
E is energy of light particle.
The distance between any two similar points of a wave is called wavelength
Figure 1
Frequency is defined as number of wavelengths of a wave that can pass through a point in one second.
Answer to Problem 7.108QP
The wavelength of light used to break per bond is
Explanation of Solution
To calculate: The wavelength of light used to break per bond.
The energy of each photon is calculated as follows,
The wave length of light used to break per bond is
The obtained wavelength is in range of near UV region of electromagnetic spectrum which corresponds to lyman series of H-atom. The minimum energy required in this region for transition corresponds to
The obtained energy is more than required energy to break the
By using the formula for energy levels of electron in H-atom, the wavelength of light used to break per bond was calculated.
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Chapter 7 Solutions
Lab Manual Experiments in General Chemistry
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