What is the energy (in kJ) of 1.00 mole of photons, each with an energy of 4.25 \times 10^{-19} J?

• A. 2.56 kJ
• B. 4.25 kJ
• C. 256 kJ
• D. 25.6 kJ

Answer: (C)

Verified step by step guidance

1. Identify the given information: the energy of one photon is \$4.25 \times 10^{-19}$ joules, and you have 1.00 mole of photons.
2. Recall that 1 mole contains Avogadro's number of particles, which is approximately \$6.022 \times 10^{23}$ photons per mole.
3. To find the total energy of 1 mole of photons, multiply the energy of one photon by Avogadro's number: \(E_{total} = (4.25 \times 10^{-19} \text{ J/photon}) \times (6.022 \times 10^{23} \text{ photons/mole})\).
4. Calculate the total energy in joules using the multiplication from the previous step (do not finalize the numeric value here).
5. Convert the total energy from joules to kilojoules by dividing by 1000, since \$1 \text{ kJ} = 1000 \text{ J}$.