Respuesta :
Energy = frequency (v) * Planck's constant (h)
E =hv
E= 6.62*10^-34 * 2.2*10^16 = 1.45*10^-17
Approximately ~ 1.5*10^-17J
E =hv
E= 6.62*10^-34 * 2.2*10^16 = 1.45*10^-17
Approximately ~ 1.5*10^-17J
Taking into account the definition of photon and energy of a photon, the correct answer is the first option: The energy of a photon with a frequency of 2.2×10¹⁶ Hz is 1.5×10⁻¹⁷ J.
You have to know that electromagnetic radiation carries energy, which can be absorbed or emitted. To explain the processes of emission and absorption, Plank and Einstein proposed that the energy of radiation is composed of indivisible units (quanta). In each elemental process only a quantum of light can be emitted or absorbed. Each of these quanta was called a "photon".
The exchanges of energy between matter and radiation take place not continuously, but by discrete and indivisible quantities or quanta of energy. The quantum of energy is proportional to the frequency of radiation.
The relationship between the amount of energy (E) transported by the photon and its frequency (f) is determined by the following expression, where the energy of a photon is obtained by multiplying Planck's constant h by the frequency f of electromagnetic radiation:
E=h×f
In this case, you know:
- h= 6.63*10⁻³⁴ Js
- f= 2.2×10¹⁶ Hz
Replacing:
E= 2.2×10¹⁶ Hz× 6.63×10⁻³⁴ Js
E= 1.4586×10⁻¹⁷ J≅ 1.5×10⁻¹⁷ J
The correct answer is the first option: The energy of a photon with a frequency of 2.2×10¹⁶ Hz is 1.5×10⁻¹⁷ J.
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