How do you solve for this solution?

Question

A liquid is exposed to infrared radiation with a wavelength of 3.71×10−4 cm. Assume that all the radiation is absorbed and converted to heat. How many photons are required for the liquid to absorb 53.97 J of heat?



number of photons =

Answer 1

E = hc/λ where E=energy; h=Plancks constant = 6.626x10^-34 Js; c=speed of light = 3x10⁸ m/s; λ=wavelength in meters = 3.71x10^-4 cm x 1 m / 100 cm = 3.71x10^-6 m

E = (6.626x10^-34 Js)(3x10⁸ m/s) / 3.71x10^-6 m

E = 5.36x10^-20 J per photon

53.97 J x 1 photon / 5.36x10^-20 J = 1.00x10²¹ photons needed