The energy of a mole of photons with frequency 6.00x10^14Hz is what in kJ?
To calculate the energy of a mole of photons with a given frequency, you can use the equation:
E = N * h * ν
Where:
E is the energy
N is Avogadro's number (6.022 × 10^23)
h is Planck's constant (6.626 × 10^(-34) J·s)
ν is the frequency of the photons
Let's calculate the energy:
E = N * h * ν
E = (6.022 × 10^23) * (6.626 × 10^(-34) J·s) * (6.00 × 10^14 Hz)
Now, let's do the calculations:
E = (6.022 × 10^23) * (6.626 × 10^(-34) J·s) * (6.00 × 10^14 Hz)
E = 2.383 × 10^(-9) J
To convert this energy from joules (J) to kilojoules (kJ), divide by 1000:
E (kJ) = (2.383 × 10^(-9) J) / 1000
E (kJ) ≈ 2.383 × 10^(-12) kJ
So, the energy of a mole of photons with a frequency of 6.00 × 10^14 Hz is approximately 2.383 × 10^(-12) kJ.