A liquid is exposed to infrared radiation with a wavelength of 5.10×10−4 cm. Assume that all the radiation is absorbed and converted to heat. How many photons are required for the liquid to absorb 42.75 J
of heat?

1.1×10²¹ photon

Explanation:

Given data:

Wavelength of radiation = 5.10×10⁻⁴ cm

How many radiations required to liquid inorder to absorbed 42.75 J = ?

Solution:

First of all we will calculate the energy of radiation having 5.10×10⁻⁴ cm.

E = h.c/ λ

E = 6.63 ×10⁻³⁴ js  × 3 ×10⁸ m/s / 0.051×10⁻⁴ m

E = 19.89 ×10⁻²⁶ j.m/ 0.051×10⁻⁴ m

E = 390 ×10⁻²² j

The energy of 1 photon with  5.10×10⁻⁴ cm. wavelength having 390 ×10⁻²² j energy.

1 photon × 42.75 J/390 ×10⁻²² j

0.11 ×10²²photon

1.1×10²¹ photon

you need to have a picture of the atom that way we can answer it