Question

) What total energy (in kJ) is contained in 1.0 mol (6.022 × 1023) of photons, all with a frequency of 2.75 × 1014 Hz

Answer #1

Answer -

The energy of a photon is **E = h*f**

where h is Planck's constant and f is the frequency of the photon.

**h= 6.62607004 × 10 ^{-34} m^{2} kg /
s**

If the frequency is f = 2.75*10^14 Hz, then the energy of one
photon is:

E = h * f

E= **6.62607004 × 10 ^{-34} m^{2} kg / s
*** 2.75 × 10

**E = 1.82*10 ^{-19} J**

If you want the energy of a mole of photons, multiply that energy by Avogadro's number.

The energy of one-mole photon =
6.022*10^{23}***1.82*10 ^{-19} J**

**The energy of the one-mole photon = 10.96
*10 ^{4} J = 109.6 kJ**

What is the the energy (in kJ/mol of photons) of infrared
radiation that has a wavelength of 26.23 micrometers? The speed of
light is 3.00x108 m/s and Planck's constant is 6.626x10-34 J*s.

How much energy is contained in 1 mol of γ-ray photons with a
wavelength of 2.68×10−5 nm

What is the wavelength (in meters) of photons with the following
energies?
93.0 kJ/mol
8.25×10−4 kJ/mol
1860 kJ/mol

Part A: The frequency of green light is
approximately 6.0*1014 s-1. The mass of an
electron is 9.11*10-31 kg. If an electron absorbs all
the energy from one photon of green light, and all of it becomes
kinetic energy for the the electron, how much more kinetic energy
will the electron have after absorbing the photon?
Part B: What is the wavelength of a photon with
the frequency 4.0*1014 Hz?
Part C: Photons with a frequency of
4.0*1014 Hz are...

What is the wavelength (in meters) of photons with the following
energies?
Part A.) 136 kJ/mol
Part C.) 4.55*10-2 kJ/mol

In a photoelectric experiment using a clean metal surface, the
maximum energy of the emitted photons was measured for a number of
different incident frequencies, with the following results.
Frequency (1014 Hz)
Energy (eV)
11.8
2.61
10.6
2.17
9.9
1.89
9.1
1.48
8.2
1.07
6.9
0.48
Plot the graph of these results and find each of the
following.
(a) Planck's constant
(b) the cutoff frequency (Hz)
(c) the work function (eV)

Calculate the energy (E) in kJ/mol corresponding to the wavelength,
486.1 nm. (Careful with units! kJ / (mol) means we have 1 mol of
photons. The Rhydberg equations or Bohr model equation give the
energy for one photon and is in J, not KJ.

Part A.
How much energy is contained in 1 mol of each of the
following?
γ-ray photons with a wavelength of 2.63×10−5
nm.
_____________ kJ/mol
Part B.
An electron traveling at 5.6×105 m/s has an uncertainty
in its velocity of 1.25×105 m/s .
What is the uncertainty in its position?
Express your answer with the appropriate units.
Δx = __________
Please help

If we have a reaction and the total bond energy is 5605 kj/ mol
for the reactants and 6900 kj/mol for the products, how do we
callculate the overall energy? also is this endothermic or
exothermic?

A laser pointer used has a frequency of 2.04* 1014 Hz.
a. What is the wavelength of the light?
b. If 23.7 KJ of energy is given off when pointing at an excited
chemical equation on the projector screen, how many photons were
emitted?

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