achieve #4 [ENDORSED]

[205696437]

Can someone help me understand this. A liquid is exposed to infrared radiation with a wavelength of 6.80×10−4 cm. Assume that all the radiation is absorbed and converted to heat. How many photons are required for the liquid to absorb 36.48 J
of heat?

[joshua_quinn_1C]

For this problem, I think you would use the wavelength to find the Energy per photon using the equation E = h(frequency) by substituting for frequency using the equation (frequency) = c/(wavelength). After you find the joules of energy per photon, you would divide 36.48 J by that value to find the amount of photons needed to get that many joules. Hopefully this helps.

[Alekhya_Pantula_2E]

Hello!
For this question you want to use the E(photon)=hc/wavelength formula to first figure out the energy of the photon and you'll be left with a number in J/photon. Then looking at the units, since you are given J and have J/photon, you can divide the energy given by the energy of the photon to be left with the number of photons.