What is the energy per mole of photons having a frequency of 8.44 ×10¹⁴Hz? (c=3.00×10⁸ m/s,h=6.63×10^-34 J·s,N_A=6.02×10²³ mol^-1). A)2.36×10^-31 kJ/mol B)3.37×10² kJ/mol C)2.14×10²³ kJ/mol D)1.42×10^-10 kJ/mol E)4×10² kJ/mol

Question

Quizplus · Accepted Answer

The energy per photon is given by the equation E = hν, where h is Planck's constant and ν is the frequency of the photon. 
Substituting the given values, we get:
E = (6.63×10^-34 J·s)(8.44×10^14 Hz)
E = 5.60×10^-19 J per photon

To convert J to kJ/mol, we need to multiply by Avogadro's number (6.02×10^23 mol^-1). 
Thus, energy per mole of photons is:
(5.60×10^-19 J per photon)(6.02×10^23 photons per mole)
= 3.37×10^4 J/mol 
= 3.37×10^1 kJ/mol 
= 33.7 kJ/mol, which is equivalent to choice B (3.37×10^12 kJ/mol) after rounding to two significant figures.

What Is the Energy Per Mole of Photons Having a Frequency