The absorption of light of frequency 1.16 × 10¹¹ Hz is required for CO molecules to go from the lowest rotational energy level to the next highest rotational energy level.Determine the energy for this transition in kJ/mol.(h = 6.626 × 10^-34 J ∙ s) A)7.69 × 10^-23 kJ/mol B)0.0463 kJ/mol C)46.3 kJ/mol D)949 kJ/mol

Question

Quizplus · Accepted Answer

The energy of the transition can be found using the equation:

ΔE = hν

where h is Planck's constant and ν is the frequency of the absorbed light.

Substituting the given values, we get:

ΔE = (6.626 × 10^-34 J ∙ s) × (1.16 × 10^11 Hz)

= 7.69 × 10^-24 J

To convert this to kJ/mol, we need to divide by Avogadro's number (6.022 × 10^23) and multiply by 10^-3:

ΔE = (7.69 × 10^-24 J/atom) / (6.022 × 10^23 atoms/mol) × 10^-3 kJ/J

= 0.0463 kJ/mol

Therefore, the correct answer is B.

The Absorption of Light of Frequency 1