Posted by **Need Help** on Sunday, December 6, 2009 at 11:51am.

Warm objects emit electromagnetic radiation in the infra-red region. Heat lamps employ this principle to generate infra-red radiation. Water absorbs infra-red radiation with wavelengths near 2.80um. Suppose this radiation is absorbed by the water and converted to heat. A 1.00 L sample of water absorbs infra-red radiation, and its temperature increases from 20C to 30C. How many photons of this radiation are used to heat the water?

- college Chemistry -
**DrBob222**, Sunday, December 6, 2009 at 11:58am
q=heat absorbed by water = mass x specific heat water x delta T. Assuming the density of water is 1.00 g/L, the mass of 1.0 L is 1,000 grams.

q = 1000 x 4.184 J/g*K x 10.

delta E = hc/wavelength.

Plug in h, c, and wavelength to calculate delta E. That is the energy per photon. Then set up a proportion to determine the number of photons required to reach q.

Post your work if you get stuck.

- college Chemistry -
**Need Help**, Sunday, December 6, 2009 at 12:23pm
Thanks for the speedy response!

Here is my work:

q = 1000 x 4.184 x 10

q = 41840

detalE = hc/wavelenght

wavelenght = 2.8 x 10^-6 m

deltaE = [(6.626 x 10^-34)(3.0 x 10^8)]/2.8 x 10^-6

delta E = 7.09 x 10^-20 m per photon

Proportion:

1 photon = 7.099 x 10^-20m

q = 41840

Therefore, 5.894 x 10^-16

Is this correct? Thanks again for you help!

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