Microwaves are used to heat food in microwave ovens. The microwave radiation is absorbed by moisture in the food. This heats the water, and as the water becomes hot, so does the food. How many photons having a wavelength of 3.00 mm would have to be absorbed by 1.45 g of water to raise its temperature by 1.00 °C?

9.06*10^22

ok

So the number of photons having a wavelength of 3.00 mm that would have to be absorbed by 1.45 g of water to raise its temperature by 1.00 °C is approximately 9.06*10^22 photons.

The table below shows the percentage of households that own a microwave in different countries. Construct a stem-and-leaf plot of the data.

Country Percent Of Household With Microwave Ovens
_____________________________________________________________
Argentina 97%
_____________________________________________________________
Belgium 93%
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Canada 69%
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Denmark 95%
______________________________________________________________
France 88%
______________________________________________________________
Germany 94%
______________________________________________________________
Greece 64%
_______________________________________________________________
Ireland 92%
________________________________________________________________
Italy 88%
________________________________________________________________
Jordan 99%
________________________________________________________________
Switzerland 91%
________________________________________________________________
United States 97%

Stem | Leaf

---- | ----
6 | 4
6 | 9
6 |
6 |
6 |
6 |
6 |
6 |
6 | 9
6 |
6 |
6 |
6 |
8 | 8
8 | 8
8 |
9 | 1
9 | 2
9 | 3
9 | 4
9 |
9 |
9 |
9 |
9 |
9 |
9 |
9 |
9 |
9 |
9 | 7
9 | 7
9 |
9 | 9
9 | 9
99 |

To determine the number of photons required to raise the temperature of water, we'll need to use the formula:

E = n * h * c / λ

where:
E is the energy,
n is the number of photons,
h is the Planck's constant (6.626 x 10^-34 J·s),
c is the speed of light (3.00 x 10^8 m/s), and
λ is the wavelength of the photons.

First, we need to calculate the energy required to raise the temperature of 1.45 g of water by 1.00 °C. We can use the specific heat capacity of water (4.18 J/g·°C) to do this:

Energy = mass * specific heat capacity * change in temperature

Energy = 1.45 g * 4.18 J/g·°C * 1.00 °C = 6.02 J

Next, we rearrange the formula to solve for the number of photons:

n = E * λ / (h * c)

Plugging in the values:

n = (6.02 J) * (3.00 mm) / [(6.626 x 10^-34 J·s) * (3.00 x 10^8 m/s)]

Now, we need to convert the wavelength from millimeters to meters:

n = (6.02 J) * (3.00 x 10^-3 m) / [(6.626 x 10^-34 J·s) * (3.00 x 10^8 m/s)]

Calculating this expression will give us the number of photons required.

E for 3.00 mm is

E = hc/wavelength. Convert wavelength in mm to m. That gives E for 1 photon which is q/photon

q needed to raise T H2O is
q = mass H2O x specific heat H2O x delta T = 1.45g x 4.184 x 1 = estimated 6 J
Then q/photon x # photons = estimated 6 and solve for # photons.