How Much Energy Do CO Molecules Need for a Rotational Transition?

[Soaring Crane]

The absorption of light of frequency 1.16 x 10^11 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 x 10-34 J s
a. 7.69 x 10-23 kJ/mol
b. 949 kJ/mol
c. 46.3 kJ/mol
d. 0.0463 kJ/mol
E = hv
= (1.16*10^11 Hz)(6.626*10^-34 J*s)
= 7.686 *10^-23 J = 7.69*10^-26 kJ* (6.02*10^23 molecules/ 1 mol) = 0.04629 kJ/mol
Thanks.

 

[Doc Al]

Looks good to me.

 

[quicknote]

I can confirm that the correct answer is option d, 0.0463 kJ/mol. This can be calculated using the formula E = hv, where E is energy, h is Planck's constant (6.626 x 10^-34 J s), and v is frequency (1.16 x 10^11 Hz). The resulting energy value is in joules, which can then be converted to kJ/mol by multiplying by Avogadro's number (6.02 x 10^23 molecules/1 mol). This gives us the energy required for the CO molecules to transition from the lowest to the next highest rotational energy level.