Given:
Density of water is 1 g/mL and volume here is 265 mL/.
So,
m = 265 g
C = 4.184 J/g.oC
Ti = 25 oC
Tf = 62 oC
use:
Q = m*C*(Tf-Ti)
Q = 265.0*4.184*(62.0-25.0)
Q = 41024 J
This is the heat required
Given:
lambda = 12 cm = 0.12 m
1st calculate energy of 1 photon
use:
E = h*c/lambda
=(6.626*10^-34 J.s)*(3.0*10^8 m/s)/(0.12 m)
= 1.657*10^-24 J
number of photon = total energy/energy of 1 photon
n = 41024.0/1.657*10^-24
= 2.477*10^28
Answer: 2.48*10^28
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Microwave ovens use microwave radiation to heat food. The microwaves are absorbed by the water molecules in the food, which is transferred to other components of the food. As the water becomes hotter, so does the food. Suppose that the microwave radiation has a wavelength of 12.4 cm . How many photons are required to heat 235 mL of coffee from 25.0 ∘C to 62.0 ∘C? Assume that the coffee has the same density, 0.997 g/mL, and specific heat capacity,...
Microwave ovens use microwave radiation to heat food. The microwaves are absorbed by the water molecules in the food, which is transferred to other components of the food. As the water becomes hotter, so does the food. Part A Suppose that the microwave radiation has a wavelength of 12.4 cm. How many photons are required to heat 285 mL of coffee from 25.0°C to 62.0 °C? Assume that the coffee has the same density, 0.997 g/mL, and specific heat capacity...
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