Wiki User
โ 13y agoE=h*f
h is Planck's constant, which is equal to 6.62 x 10-34 J . s.
f is the frequency in Hz.
Multiplication of two numbers together is left as an exercise to the student.
3.2 x 10-18 J
acutual answer on The Question is 4.3 x 10-19J
Wiki User
โ 14y agoThe energy of a photon can be calculated using the equation E = hf, where h is the Planck constant (6.626 x 10^-34 J*s) and f is the frequency. Plugging in the values, the energy of a photon with a frequency of 4 x 10^8 Hz is approximately 2.65 x 10^-25 Joules.
Wiki User
โ 10y agoThe energy of a photon of frequency 1.25 x 10^6 Hz can be calculated using the relation E = hf, where E is the energy in Joules, h is Planck's constant 6.63 x 10^-34 m^2 kg / s, and f is the frequency in cycles per second (Hz). The energy of this photon is 8.28 x 10^-28 J.
Wiki User
โ 13y agoTo calculate this we use the de Broglie equation f=E/h, where f is the frequency, E is the energy of the particle and h is Planck's constant.
The energy of a photon with a frequency of 4100000000 Hz then equals:
E= f*h = 4100000000 Hz * 6.626068 * 10^-34 Js = 2.71*10^-24 J
pitch. A higher frequency sound will be perceived as having a higher pitch, whereas a lower frequency sound will be perceived as having a lower pitch.
Ok, so this goes back to the inverse relationship between wavelength and frequency ( energy). As wavelength increases , frequency decreases, the relationship between the two is a inverse relationship. the Red light, wavelength of approx. 700 m^-7 , has a greater wavelength then of the blue light, 400m ^-7. This means , due to frequency and wavelength having an inverse relationship, blue light has a greater frequency (energy) than red light. This is why blue light, no matter how dim, will impart more energy to an electron , then a red light would.
In visible light, color is an indication of the wavelength of light that is being reflected or emitted by an object. Different colors correspond to different wavelengths of light, with red having the longest wavelength and violet having the shortest.
The visible light frequency bandwidth ranges from approximately 430 to 750 terahertz, corresponding to wavelengths from about 400 to 700 nanometers. This range includes the colors of the rainbow, with red having the longest wavelength and lowest frequency, and violet having the shortest wavelength and highest frequency.
Proton.
The energy of a photon can be calculated using the formula E = hf, where h is Planck's constant (6.626 x 10^-34 Jยทs) and f is the frequency of the photon. Plugging in the values, the energy of a photon with a frequency of 4 x 10^7 Hz is approximately 2.65 x 10^-26 Joules.
The energy of light is related to its frequency, with higher frequency light having higher energy. This relationship is described by Planck's equation, E = h*f, where E is energy, h is Planck's constant, and f is frequency.
The energy is 3,8431.10e-14 joule.
The frequecy is o,74958 Hz.
The frequency of radiation refers to the number of wave cycles that pass a given point in one second. It is closely related to the energy of the radiation, with higher frequency radiation having higher energy levels. Radiation with higher frequency can be more harmful to living organisms.
The frequency of a photon can be calculated using the formula E = hf, where E is the energy of the photon, h is Planck's constant (6.626 x 10^-34 Js), and f is the frequency. Rearranging the formula to solve for frequency gives f = E/h. Substituting the given energy value of 5 x 10^-24 J gives a frequency of approximately 7.55 x 10^9 Hz.
Red light has lower energy than yellow light. The energy of a light wave is directly proportional to its frequency, with red light having a lower frequency and therefore lower energy compared to yellow light.
To calculate the energy of a photon, we can use the equation E = hf, where E is the energy, h is Planck's constant (6.626 x 10^-34 Js), and f is the frequency of the photon. Plugging in the values: E = 6.626 x 10^-34 Js * 4 x 10^7 Hz = 2.65 x 10^-26 J. Therefore, the approximate energy of the photon is 2.65 x 10^-26 joules.
If the photon is having very less frequency (say v=1Hz) ,then the Energy of such photon will be the smallest one. It can be inferred that the smallest unit of light energy will correspond to the smallest frequency of such quanta. But from the uncertainty principle it limits the energy of a quanta.
The types of electromagnetic waves that exist include radio waves, microwaves, infrared, visible light, ultraviolet, X-rays, and gamma rays. These waves vary in frequency and energy, with radio waves having the lowest frequency and energy, and gamma rays having the highest.
A wave with high energy is characterized by having a high amplitude and frequency, which means it carries a lot of energy per unit time. This type of wave can be more destructive and have a greater impact than waves with lower energy levels.
they do not possess enough energy in their individual particles, known as photons, to overcome the work function of the metal and eject electrons. The energy of the photons is directly related to their frequency, with higher frequency light having greater energy. This is why only light with sufficient energy, typically ultraviolet or higher frequency, can eject electrons from metals in the photoelectric effect.