Question

Water is exposed to infrared radiation with a wavelength of 2.15×10-4 cm. A. What is the frequency of a photon of that wavelength? B. What is the energy of a photon of that wavelength? C. When water absorbs energy, 4.184J of energy are required to raise the temperature of 1.000 gram of water by 1.000°C. Assuming all the energy is absorbed by the water and converted to heat, how many moles of photons are required to raise the temperature of 15.80g of water from 3.5°C to 38.7°C?

          Water is exposed to infrared radiation with a wavelength of 2.15×10-4 cm. A. What is the frequency of a photon of that wavelength? B. What is the energy of a photon of that wavelength? C. When water absorbs energy, 4.184J of energy are required to raise the temperature of 1.000 gram of water by 1.000°C. Assuming all the energy is absorbed by the water and converted to heat, how many moles of photons are required to raise the temperature of 15.80g of water from 3.5°C to 38.7°C?

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