Answer :
Final answer:
The energy associated with infrared light having a wavelength of 1.55 x 10⁻⁶ m is 9.93 kJ/mol.
Explanation:
The energy associated with infrared light can be calculated using the formula E = hc/λ, where E is the 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), and λ is the wavelength of the light. To convert this energy to kJ/mole, we need to use Avogadro's constant (6.022 x 10^23 molecules/mol). First, calculate the energy in J/mol:
E = (6.626 x 10^-34 J·s) * (3.00 x 10^8 m/s) / (1.55 x 10^-6 m) = 1.85 x 10^-19 J
Then, convert this energy to kJ/mol:
E_kJ/mol = (1.85 x 10^-19 J) / (1000 J/kJ) * (6.022 x 10^23 molecules/mol) = 9.93 kJ/mol
Therefore, the energy associated with infrared light having a wavelength of 1.55 x 10^-6 m is 9.93 kJ/mol.
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