Math  /  Algebra

Question2) What is the energy in joules, of one mole of photons associated with vissible light having a wavelength of 486.1 nm ? A) 12.41 kJ B) 2.461×104 J2.461 \times 10^{-4} \mathrm{~J} C) 2.461×105 J2.461 \times 10^{5} \mathrm{~J} D) 6.167×1014 J6.167 \times 10^{14} \mathrm{~J} E) 8.776×1025 J8.776 \times 10^{25} \mathrm{~J}

Studdy Solution
Calculate the energy of one mole of photons by multiplying the energy of a single photon by Avogadro's number:
Emole=(4.090×1019J)×(6.022×1023mol1) E_{\text{mole}} = (4.090 \times 10^{-19} \, \text{J}) \times (6.022 \times 10^{23} \, \text{mol}^{-1})
Emole=2.461×105J/mol E_{\text{mole}} = 2.461 \times 10^{5} \, \text{J/mol}
The energy of one mole of photons is:
2.461×105J \boxed{2.461 \times 10^{5} \, \text{J}}
Therefore, the correct answer is option C.

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