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16) How many photons are contained in a burst of yellow light (589 nm) from a sodium lamp that contains 609 kJ of energy?
A) 3.37 × 1019 photons
B) 3.06 × 1030 photons
C) 1.81 × 1024 photons
D) 4.03 × 1028 photons
E) 2.48 × 1025 photons

Respuesta :

The correct answer to this question is this one:

find the energy of one photon:

E=h*c/λ

divide the energy given by the energy of one photon of that wavelength

What I've done so far is convert wave length to m and energy to j. 

E photon = h * x / wave length
E = (6.626 x 10^-43)(3.00 x 10^8) / 587 ^ -9  = 3.38 x 10 ^18 J
3.38 x 10 ^18 J x 1000 kj / 1 j = 3.37 x 10 ^ 16 Kj
609 kJ/  3.37 x 10 ^ 16 Kj =  1.81 x 10 ^ 16

E = (6.626 x 10^-34)(3.00 x 10^8) / 587 ^ -9 = 3.38 x 10 ^19 J
3.38 x 10 ^19 J x 1000 kj / 1 j = 3.37 x 10 ^ -16 Kj
609 kJ/ 3.37 x 10 ^ 16 Kj = 1.81 x 10 ^ 18 but the answer is  1.81 × 10^24 photons

3.38 x 10 ^-19 J
should be negative

then 3.38 x 10 ^18 J x 1kJ/1000 J

you're converting from J to kJ.. just like meters to kilometres, you wouldn't multiply you would divide

Answer:  C) [tex]1.81\times 10^{24}[/tex] photons

Explanation:

[tex]E=\frac{nhc}{\lambda}[/tex]

E= energy = 609 kJ = 609000 J    (1kJ=1000J)

[tex]n[/tex] = number of photons = ?

h = Planck's constant  = [tex]6.626\times 10^{-34}Js[/tex]

c = speed of light = [tex]3\times 10^8m/s[/tex]

[tex]\lambda[/tex] = wavelength of photon = 589 nm =[tex]589\times 10^{-9}m[/tex]

Putting values in above equation, we get:

[tex]609000J=\frac{n\times (6.626\times 10^{-34}Js)\times (3\times 10^8m/s)}{589\times 10^{-9}m}[/tex]

[tex]n=1.81\times 10^{24}[/tex]

Thus there are [tex]1.81\times 10^{24}[/tex] photons in a burst of yellow light (589 nm) from a sodium lamp that contains 609 kJ of energy.

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