Determine the energy of 1.70 mol of photons for each of the following kinds of light. (Assume three significant figures.)PART A infrared radiation (1600 nm)PART B visible light (505 nm )PART C ultraviolet radiation (150 nm )

For A: The energy of the given amount of photons for infrared radiation is

For B: The energy of the given amount of photons for infrared radiation is

For C: The energy of the given amount of photons for infrared radiation is

Explanation:

The relationship between energy and frequency is given by Planck's equation, which is:

       ......(1)

where,

h = Planck's constant  =

E = energy of the light

c = speed of light =

= wavelength of light

= Avogadro's number =

n = number of moles of photons = 1.70 moles

Conversion factor used:  

Wavelength of infrared radiation =

Putting values in equation 1, we get:

Hence, the energy of the given amount of photons for infrared radiation is

Wavelength of visible light =

Putting values in equation 1, we get:

Hence, the energy of the given amount of photons for infrared radiation is

Wavelength of ultraviolet radiation =

Putting values in equation 1, we get:

Hence, the energy of the given amount of photons for infrared radiation is

the ratio of the conjugate base to the acid required to attain the desired ph.