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The number of photons of light of barv ...

The number of photons of light of `barv =3.5×10^6m^(−1)` necessary to provide 2 J of energy are:

A

`6xx10^(17)`

B

`2.87xx10^(18)`

C

`6xx10^(-17)`

D

`2.87xx10^(-18)`

Text Solution

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The correct Answer is:
To solve the problem of finding the number of photons of light required to provide 2 J of energy with a wave number of \( \bar{\nu} = 3.5 \times 10^6 \, \text{m}^{-1} \), we can follow these steps: ### Step 1: Understand the relationship between energy, number of photons, and wave number The energy \( E \) provided by \( n \) photons can be expressed as: \[ E = n \cdot h \cdot \nu \] where: - \( E \) is the total energy (in joules), - \( n \) is the number of photons, - \( h \) is Planck's constant (\( 6.626 \times 10^{-34} \, \text{J s} \)), - \( \nu \) is the frequency of the light. ### Step 2: Relate wave number to frequency The wave number \( \bar{\nu} \) is related to the wavelength \( \lambda \) by: \[ \bar{\nu} = \frac{1}{\lambda} \] The frequency \( \nu \) can be related to the wave number by: \[ \nu = c \cdot \bar{\nu} \] where \( c \) is the speed of light (\( 3 \times 10^8 \, \text{m/s} \)). ### Step 3: Substitute frequency into the energy equation Substituting \( \nu \) into the energy equation gives: \[ E = n \cdot h \cdot (c \cdot \bar{\nu}) \] Rearranging this to find \( n \): \[ n = \frac{E}{h \cdot c \cdot \bar{\nu}} \] ### Step 4: Substitute the known values Now we can substitute the known values into the equation: - \( E = 2 \, \text{J} \) - \( h = 6.626 \times 10^{-34} \, \text{J s} \) - \( c = 3 \times 10^8 \, \text{m/s} \) - \( \bar{\nu} = 3.5 \times 10^6 \, \text{m}^{-1} \) So, \[ n = \frac{2}{(6.626 \times 10^{-34}) \cdot (3 \times 10^8) \cdot (3.5 \times 10^6)} \] ### Step 5: Calculate the value of \( n \) Calculating the denominator: \[ (6.626 \times 10^{-34}) \cdot (3 \times 10^8) \cdot (3.5 \times 10^6) = 6.626 \times 3 \times 3.5 \times 10^{-34 + 8 + 6} \] Calculating the numerical part: \[ 6.626 \times 3 \times 3.5 \approx 69.5 \] Thus, the denominator becomes: \[ 69.5 \times 10^{-20} = 6.95 \times 10^{-19} \] Now substituting back into the equation for \( n \): \[ n = \frac{2}{6.95 \times 10^{-19}} \approx 2.877 \times 10^{18} \] ### Final Answer The number of photons required is approximately: \[ n \approx 2.877 \times 10^{18} \]

To solve the problem of finding the number of photons of light required to provide 2 J of energy with a wave number of \( \bar{\nu} = 3.5 \times 10^6 \, \text{m}^{-1} \), we can follow these steps: ### Step 1: Understand the relationship between energy, number of photons, and wave number The energy \( E \) provided by \( n \) photons can be expressed as: \[ E = n \cdot h \cdot \nu \] where: ...
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