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Ket [755]
3 years ago
10

A laser produces 17.0 mW of light. In 4.00 hr , the laser emits 6.04×1020 photons. What is the wavelength of the laser?

Chemistry
2 answers:
Vlad [161]3 years ago
5 0
The unit 'mW' means milliwatts. It is a unit of work. There are 1,000 milliwatts in a 1 Watt of work. In 4 hours, there are 14,400 seconds.

Work= Energy/time
17 mW * 1 W/1000 mW = Energy/(14,400 seconds)
Solving for energy,
Energy = 244.8 J
Energy/photon = 244.8 J/(6.04×10²⁰) = 4.053×10⁻¹⁹ J/photon

Using the Planck's equation:

E = hc/λ
where h = 6.626×10⁻³⁴ m²·kg/s, c = 3,00,000,000 m/s and λ is the wavelength

4.053×10⁻¹⁹ J/photon = (6.626×10⁻³⁴ m²·kg/s)(3,00,000,000 m/s)/λ
λ = 4.9×10⁻⁷ m or 49 micrometers


jarptica [38.1K]3 years ago
3 0

Answer:

λ = 490.81 nm

Explanation:

The first thing we need to do is use the correct units. Let's convert the mW to J/s.

1 Watt --------> 1 J/s

And we have 17 mW:

1 Watt --------> 1000 mW

Therefore, converting the mili watts to J/s we have:

17 mW * 1 J/s / 1000 mW = 0.017 J/s

Now, we have 4 hours, and in 1 hour we have 3600 seconds so:

t = 4 * 3600 = 14,400 s

Now, the expression to calculate the wavelength is the following:

E = hc/λ (1)

Where:

E: Energy emmited by the laser by photons (J)

h: Planck constant = 6.626x10⁻³⁴ J.s

c: speed of light = 3x10⁸ m/s

λ: wavelength (nm)

Now, we have the Power of the laser, but not the energy emmited by photons. Let's calculate that value:

E = 0.017 J/s * 14,400 s / 6.04x10²⁰

E = 4.05x10⁻¹⁹ J

Now that we have the value of Energy, we just solve for Lambda from (1) to get the wavelength:

λ = hc/E (2)

Now, all we have to do is replace the obtained values and solve for the wavelength:

λ = (6.626x10⁻³⁴ J.s * 3x10⁸ m/s) / 4.05x10⁻¹⁹ J

λ = 490.81x10⁻⁹ m

And to get this value to nanometers (The usual unit of wavelength):

1 m ------> 1x10⁹ nm

Therefore:

<h2><em><u>λ = 490.81 nm</u></em></h2>
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Answer :

(a) The pressure of the vapor in the flask in atm is, 0.989 atm

(b) The temperature of the vapor in the flask in Kelvin is, 372.7 K

    The volume of the flask in liters is, 0.2481 L

(c) The mass of vapor present in the flask was, 0.257 g

(d) The number of moles of vapor present are 0.00802 mole.

(e) The mass of one mole of vapor is 32.0 g/mole

Explanation : Given,

Mass of empty flask and stopper = 55.844 g

Volume of liquid = 5 mL

Temperature = 99.7^oC

Mass of flask and condensed vapor = 56.101 g

Volume of flask = 248.1 mL

Barometric pressure in the laboratory = 752 mmHg

(a) First we have to determine the pressure of the vapor in the flask in atm.

Pressure of the vapor in the flask = Barometric pressure in the laboratory = 752 mmHg

Conversion used :

1atm=760mmHg

or,

1mmHg=\frac{1}{760}atm

As, 1mmHg=\frac{1}{760}atm

So, 752mmHg=\frac{752mmHg}{1mmHg}\times \frac{1}{760}atm=0.989atm

Thus, the pressure of the vapor in the flask in atm is, 0.989 atm

(b) Now we have to determine the temperature of the vapor in the flask in Kelvin.

Conversion used :

K=273+^oC

As, K=273+^oC

So, K=273+99.7=372.7

Thus, the temperature of the vapor in the flask in Kelvin is, 372.7 K

Now we have to determine the volume of the flask in liters.

Conversion used :

1 L = 1000 mL

or,

1 mL = 0.001 L

As, 1 mL = 0.001 L

So, 248.1 mL = 248.1 × 0.001 L = 0.2481 L

Thus, the volume of the flask in liters is, 0.2481 L

(c) Now we have to determine the mass of vapor that was present in the flask.

Mass of flask and condensed vapor = 56.101 g

Mass of empty flask and stopper = 55.844 g

Mass of vapor in flask = Mass of flask and condensed vapor - Mass of empty flask and stopper

Mass of vapor in flask = 56.101 g - 55.844 g

Mass of vapor in flask = 0.257 g

Thus, the mass of vapor present in the flask was, 0.257 g

(d) Now we have to determine the number of moles of vapor present.

Using ideal gas equation:

PV = nRT

where,

P = Pressure of vapor = 0.989 atm

V = Volume of vapor  = 0.2481 L

n = number of moles of vapor = ?

R = Gas constant = 0.0821 L.atm/mol.K

T = Temperature of vapor = 372.7 K

Putting values in above equation, we get:

(0.989atm)\times 0.2481L=n\times (0.0821L.atm/mol.K)\times 372.7K\\\\n=0.00802mole

Thus, the number of moles of vapor present are 0.00802 mole.

(e) Now we have to determine the mass of one mole of vapor.

\text{Mass of one mole of vapor}=\frac{\text{Mass of vapor}}{\text{Moles of vapor}}

\text{Mass of one mole of vapor}=\frac{0.257g}{0.00802mole}=32.0g/mole

Thus, the mass of one mole of vapor is 32.0 g/mole

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