Question

How to solve 600.0 mL of air is at 20.0 °C.What is the volume at 60.0 °C?​

Answer 1

Explanation:

Every photon has a characteristic energy associated with it. The energy of a photon is dependent on its frequency. The way I would solve this is to convert the wavelength, 679 nm, to a frequency and then find the energy. After we know the energy of a single photon, we can find out how many it takes to get the total energy of the pulse (0.528 J).

Some useful equations:

λν = c

Wavelength, λ (lambda), times frequency, ν (nu), equals the speed of light.

c = 3.0 x 108 m/s.

E = hν

Energy of a single photon is the product of Planck's constant, h, and the frequency, ν. h = 6.63 x 10-34 J•s.

I prefer to manipulate the equations before plugging in our known values.

We have a wavelength as a known, so let's solve for the energy of a single photon at that wavelength:

λν = c

ν = c/λ

Plug this into the other equation:

E = hν

E = hc/λ

Now we can plug in our two constants (h and c, they never change) and our known (λ = 679 nm = 679 x 10-9 m) and find the energy of a single photon. Make sure you use the value of the wavelength in meters (679 x 10-9 m).

E = 2.93 x 10-19

Let's check our units:

h is in J•s (energy • time). c is in m/s (distance/time). Wavelength is in m (after we converted from nm).

So our final units should be: (J•s•m/s)/m = (J•s•m/s)/m = (J•m)/m = J

Good, that is what we wanted.

Each photon of light at 679 nm is 2.93 x 10-19 J of energy. The whole pulse is 0.528 J. It is a simple matter of division to get:

0.528 J / 2.93 x 10-19 J = 1.8 x 1018 photons

We divided the energy of the whole pulse by the energy per photon to get the number of photons.

Feel free to comment on the areas which are confusing. Good luck.