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## How do you calculate one photon?

The energy of a single photon is: **hν or = (h/2π)ω** where h is Planck’s constant: 6.626 x 10-34 Joule-sec.

## How much energy is 3 moles photons?

Each photon has an energy of 2.9450×10^{–}^{19} J. 1 mol of a photon has 6.022×10^{23} photons. The answer is option A), In 3.00 moles of photons with a wavelength of 675 nm, the energy is **532 kJ**.

## How do you find the moles of photons?

To find the energy of a photon, multiply Planck’s constant by the speed of light, then divide by the photon’s wavelength. For a mole of photons, **multiply the result by Avogadro’s number**.

## What is the energy of 0.10 mol of these photons?

14 -1Step-2(b) Here we have to calculate the energy of 0.10 mol of these photons . It is known that energy can be calculated as E = h 14 -1 = 6.626×10-34 J.s ×5.09×10 s = 3.37×10 -19JFor 0.10 mol of photon = 3.37×10 -19J×0.10×6.023×10 =20297.5JThus the energy of 0.10 mol of photon is found to be **20297.5 J/photon**.

## How many joules is a photon?

It should not surprise us that the energy of a single photon is small. It is also useful to calculate the number of photons in a Joule of energy. This is just the inverse of the energy per photon, and gives **3.2×10 ^{18} photons per Joule**.

## How do you calculate energy per mole of photons?

The equation used to find the energy in a mole of photons is **E= hc/lambda** where h is Planck’s constant, c is the speed of light and is the wavelength of light.

## What is the equation for the energy of 1 photon when the calculation must be done using the wavelength of light?

The energy of a single photon is given by **E=hν=hcλ**.

## What is the frequency of a photon?

The frequency of a photon is defined as **how many wavelengths a photon propagates each second**. Unlike an electromagnetic wave, a photon cannot actually be of a color. Instead, a photon will correspond to light of a given color.

## How do you go from kJ mol to J photon?

The conversion to kJ/mol involves using Avogadro’s number and converting J to kJ: **E (kJ/mol) =** (3.71_{3} × 10^{−}^{19} J/photon)(6.022 × 10^{23} photon/mol)(10^{−}^{3}kJ/J) = 224 kJ/mol.

## How do you convert photons to joules?

The equation for determining the energy of a photon of electromagnetic radiation is **E=hν** , where E is energy in Joules, h is Planck’s constant, 6.626×10−34J⋅s , and ν (pronounced “noo”) is the frequency.

## How many photons are in a laser pulse?

A typical laser pulse used in MALDI is about 60 microjoule / pulse at 337 nm. At 337 nm the energy is about 6 x 10^-19 J/photon. Doing the math suggests that **about 10^14 photons** are in a typical desorption pulse.