Final answer:
The energy of microwave radiation with a frequency of 1.23 × 10^11 Hz is approximately 8.16 × 10^-23 J per photon.
Step-by-step explanation:
To calculate the energy of a photon, we use the equation E = hf, where E represents energy, h is Planck's constant (6.626 × 10^-34 J·s), and f denotes frequency. This equation, developed by physicist Max Planck, relates the energy of a photon to its frequency.
In the given scenario, we have a frequency of 1.23 × 10^11 Hz. By substituting this value into the equation, we can determine the energy:
E = (6.626 × 10^-34 J·s) × (1.23 × 10^11 Hz) = 8.16 × 10^-23 J per photon.
This calculation shows that the energy of the microwave radiation is approximately 8.16 × 10^-23 J per photon. This value represents the amount of energy carried by each individual microwave photon.
Planck's constant, denoted by h, is a fundamental constant in physics. It quantifies the relationship between the energy and frequency of a photon. Its value, 6.626 × 10^-34 J·s, plays a crucial role in understanding the behavior and interactions of light on a quantum level.
By utilizing the equation E = hf, scientists and researchers can calculate the energy of photons across various electromagnetic spectra. This knowledge is essential in various fields, including quantum physics, optics, and telecommunications.
In summary, the energy of a photon can be calculated using the equation E = hf, with E representing energy, h representing Planck's constant, and f representing frequency. In the case of microwave radiation with a frequency of 1.23 × 10^11 Hz, the energy is approximately 8.16 × 10^-23 J per photon.