A container with 0.317 L of water is placed into microwave and is then radiated with electromagnetic energy that has a wavelength of 13.3 cm. The temperature of the water then rose by 74.3 °C. Calculate the number of photons that were absorbed by the water. Assume water has a density of 1.00 g·mL-1 and its specific heat is 4.184 J·g-1·°C-1

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Eaton

Chemistry

20 September, 23:36

A container with 0.317 L of water is placed into microwave and is then radiated with electromagnetic energy that has a wavelength of 13.3 cm. The temperature of the water then rose by 74.3 °C. Calculate the number of photons that were absorbed by the water. Assume water has a density of 1.00 g·mL-1 and its specific heat is 4.184 J·g-1·°C-1

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Trystan Salazar · Answer 1

E = h * c / lambda where

E is the energy

h is Plack's constant, h = 6.626 * 10 - 34 joule·s

c is the speed of light in m/sec

lambda is the wavelength.

The total energy required = mass of water * specific heat * temperature change

Divide the total energy by the energy per photon.