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It has been found that gaseous iodine molecule just dissociates into iodine atoms after absorption of light at wavelengths 4995armstrong. The energy required to dissociate 1 mole of iodine molecules is?? Options: 1. 52.2 K Cal/mole 2. 93.4 K Cal/mole 3. 63.4 K cal/ mole 4. 57.3 K cal/ mole?
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It has been found that gaseous iodine molecule just dissociates into i...
Energy required to dissociate gaseous iodine molecules
To calculate the energy required to dissociate 1 mole of iodine molecules, we need to use the concept of wavelength and energy.
1. Understanding the absorption of light by iodine molecules:
- When iodine molecules absorb light at a specific wavelength, they gain energy.
- This energy can cause the breaking of the bond between the two iodine atoms, resulting in the dissociation of the molecule into iodine atoms.
2. Applying the concept of wavelength and energy:
- The given wavelength is 4995 Å (Angstroms).
- To determine the energy of light at this wavelength, we can use the equation: E = hc/λ.
- E represents energy
- h is Planck's constant (6.626 x 10^-34 J·s)
- c is the speed of light (3.00 x 10^8 m/s)
- λ is the wavelength in meters
- Converting the given wavelength to meters: 4995 Å = 4995 x 10^-10 m.
- Substituting the values into the equation, we get: E = (6.626 x 10^-34 J·s) * (3.00 x 10^8 m/s) / (4995 x 10^-10 m).
3. Calculating the energy:
- Simplifying the equation, we have: E = 3.98 x 10^-19 J.
- Now, we need to convert this energy to kilocalories per mole.
- 1 Joule is equal to 0.000239 Kcal.
- Therefore, the energy in Kcal is: (3.98 x 10^-19 J) * (0.000239 Kcal/J).
- Simplifying the equation, we get: 9.52 x 10^-23 Kcal.
- Since we are interested in the energy required to dissociate 1 mole of iodine molecules, we can multiply the energy by Avogadro's number (6.022 x 10^23):
- (9.52 x 10^-23 Kcal) * (6.022 x 10^23).
- Simplifying the equation, we have: 57.3 Kcal/mol.
4. Answer:
The energy required to dissociate 1 mole of iodine molecules is 57.3 Kcal/mol.
To calculate the energy required to dissociate 1 mole of iodine molecules, we need to use the concept of wavelength and energy.
1. Understanding the absorption of light by iodine molecules:
- When iodine molecules absorb light at a specific wavelength, they gain energy.
- This energy can cause the breaking of the bond between the two iodine atoms, resulting in the dissociation of the molecule into iodine atoms.
2. Applying the concept of wavelength and energy:
- The given wavelength is 4995 Å (Angstroms).
- To determine the energy of light at this wavelength, we can use the equation: E = hc/λ.
- E represents energy
- h is Planck's constant (6.626 x 10^-34 J·s)
- c is the speed of light (3.00 x 10^8 m/s)
- λ is the wavelength in meters
- Converting the given wavelength to meters: 4995 Å = 4995 x 10^-10 m.
- Substituting the values into the equation, we get: E = (6.626 x 10^-34 J·s) * (3.00 x 10^8 m/s) / (4995 x 10^-10 m).
3. Calculating the energy:
- Simplifying the equation, we have: E = 3.98 x 10^-19 J.
- Now, we need to convert this energy to kilocalories per mole.
- 1 Joule is equal to 0.000239 Kcal.
- Therefore, the energy in Kcal is: (3.98 x 10^-19 J) * (0.000239 Kcal/J).
- Simplifying the equation, we get: 9.52 x 10^-23 Kcal.
- Since we are interested in the energy required to dissociate 1 mole of iodine molecules, we can multiply the energy by Avogadro's number (6.022 x 10^23):
- (9.52 x 10^-23 Kcal) * (6.022 x 10^23).
- Simplifying the equation, we have: 57.3 Kcal/mol.
4. Answer:
The energy required to dissociate 1 mole of iodine molecules is 57.3 Kcal/mol.
Community Answer
It has been found that gaseous iodine molecule just dissociates into i...
(4). 57.3 k cal/ mole
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It has been found that gaseous iodine molecule just dissociates into iodine atoms after absorption of light at wavelengths 4995armstrong. The energy required to dissociate 1 mole of iodine molecules is?? Options: 1. 52.2 K Cal/mole 2. 93.4 K Cal/mole 3. 63.4 K cal/ mole 4. 57.3 K cal/ mole?
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It has been found that gaseous iodine molecule just dissociates into iodine atoms after absorption of light at wavelengths 4995armstrong. The energy required to dissociate 1 mole of iodine molecules is?? Options: 1. 52.2 K Cal/mole 2. 93.4 K Cal/mole 3. 63.4 K cal/ mole 4. 57.3 K cal/ mole? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about It has been found that gaseous iodine molecule just dissociates into iodine atoms after absorption of light at wavelengths 4995armstrong. The energy required to dissociate 1 mole of iodine molecules is?? Options: 1. 52.2 K Cal/mole 2. 93.4 K Cal/mole 3. 63.4 K cal/ mole 4. 57.3 K cal/ mole? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for It has been found that gaseous iodine molecule just dissociates into iodine atoms after absorption of light at wavelengths 4995armstrong. The energy required to dissociate 1 mole of iodine molecules is?? Options: 1. 52.2 K Cal/mole 2. 93.4 K Cal/mole 3. 63.4 K cal/ mole 4. 57.3 K cal/ mole?.
It has been found that gaseous iodine molecule just dissociates into iodine atoms after absorption of light at wavelengths 4995armstrong. The energy required to dissociate 1 mole of iodine molecules is?? Options: 1. 52.2 K Cal/mole 2. 93.4 K Cal/mole 3. 63.4 K cal/ mole 4. 57.3 K cal/ mole? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about It has been found that gaseous iodine molecule just dissociates into iodine atoms after absorption of light at wavelengths 4995armstrong. The energy required to dissociate 1 mole of iodine molecules is?? Options: 1. 52.2 K Cal/mole 2. 93.4 K Cal/mole 3. 63.4 K cal/ mole 4. 57.3 K cal/ mole? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for It has been found that gaseous iodine molecule just dissociates into iodine atoms after absorption of light at wavelengths 4995armstrong. The energy required to dissociate 1 mole of iodine molecules is?? Options: 1. 52.2 K Cal/mole 2. 93.4 K Cal/mole 3. 63.4 K cal/ mole 4. 57.3 K cal/ mole?.
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It has been found that gaseous iodine molecule just dissociates into iodine atoms after absorption of light at wavelengths 4995armstrong. The energy required to dissociate 1 mole of iodine molecules is?? Options: 1. 52.2 K Cal/mole 2. 93.4 K Cal/mole 3. 63.4 K cal/ mole 4. 57.3 K cal/ mole?, a detailed solution for It has been found that gaseous iodine molecule just dissociates into iodine atoms after absorption of light at wavelengths 4995armstrong. The energy required to dissociate 1 mole of iodine molecules is?? Options: 1. 52.2 K Cal/mole 2. 93.4 K Cal/mole 3. 63.4 K cal/ mole 4. 57.3 K cal/ mole? has been provided alongside types of It has been found that gaseous iodine molecule just dissociates into iodine atoms after absorption of light at wavelengths 4995armstrong. The energy required to dissociate 1 mole of iodine molecules is?? Options: 1. 52.2 K Cal/mole 2. 93.4 K Cal/mole 3. 63.4 K cal/ mole 4. 57.3 K cal/ mole? theory, EduRev gives you an
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