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Photochemistry & Beer-Lambert's Law | Physical Chemistry PDF Download

Photochemistry

Photochemistry process involves the initiation of a chemical reaction through the absorption of a photon by an atom or molecule.

  • When a molecule absorbs a photon of light, the energy of photon is transferred to the molecule. The energy of a photon is given by the Planck equation:

Photochemistry & Beer-Lambert`s Law | Physical Chemistry

h = Planck constant = 6.626 × 10–34 J-s
c = speed of light in vacuum = 3 × 108 ms–1
v = frequency of light
and λ = wavelength of light

 Photochemistry & Beer-Lambert`s Law | Physical Chemistry

So, S1, S2, T1 & T2 are electronic levels.
S → singlet
T → triplet

  • Radiative Transition: Loss of excess electronic energy through the emission of a photon is known as radiative transition.
  •  Fluorescence: The process by which photons are emitted in radiative transit io n between S1 and S0 is known as fluorescence.
  • Phosphorescence: The process by which photons are emitted in radiative transit io n between T1 and S0 is known as phosphorescence.
  • The lifetime for phosphorescence is longer (10–6 s) than fluorescence (10–9 s) Photophysical reactions are corresponding rate expressions.

Photochemistry & Beer-Lambert`s Law | Physical Chemistry

  • Quantum Yield: Photochemistry & Beer-Lambert`s Law | Physical Chemistry

 Photochemistry & Beer-Lambert`s Law | Physical Chemistry


The Beer-Lambert Law.

The Beer-Lambert law states that for a given material sample path length and concentration of the sample are directly proportional to the absorbance of the light.

Photochemistry & Beer-Lambert`s Law | Physical Chemistry

  • Beer-Lambert Law derivation helps us to define the relationship of the intensity of visible UV radiation with the exact quantity of substance present. 
  • The derivation of Beer-Lambert Law has many applications in modern-day science. Used in modern-day labs for testing of medicines, organic chemistry, and to test with quantification. These are some fields that this law finds its uses in.
  • When a beam of monochromatic radiation of a suitable frequency passes through a solution, it is absorbed by the solution.

Question for Photochemistry & Beer-Lambert's Law
Try yourself:What is the process by which excess electronic energy is lost through the emission of a photon?
View Solution

The Beer-Lambert law is expressed as:

A = εLc

where,

  • A is the amount of light absorbed for a particular wavelength by the sample
  • ε is the molar extinction coefficient
  • L is the distance covered by the light through the solution
  • c is the concentration of the absorbing species

But Beer-Lambert law is a combination of two different laws: Beer’s law and Lambert law.


Derivation of Absorbance and Transmittance

Photochemistry & Beer-Lambert`s Law | Physical Chemistry

I0 = intensit y of incident light
I = intensity of transmitted light
and Ia = Intensity of the light absorbed = I0 – I
Absorbance of solution, A =  Photochemistry & Beer-Lambert`s Law | Physical Chemistry

A = Photochemistry & Beer-Lambert`s Law | Physical Chemistry         …(1)

where A = absorbance
C = concentration of solution
∈ = molar extinction coefficient or molar absorption coefficient (unit = concentration length–1)
l = path length

Transmittance;           

T = Photochemistry & Beer-Lambert`s Law | Physical Chemistry

T =Photochemistry & Beer-Lambert`s Law | Physical Chemistry…(2)

The absorbance of a solution is additive whereas the transmittance is multiplicative.

Some Important Questions

Q.1. A monochromatic light is an incident on the solution of 0.05 molar concentration of an absorbing substance. The intensity of the radiation is reduced to one-fourth of the initial value after passing through 10 cm length of the solution. Calculate the molar extinction coefficient of the substance.
 Sol.
From bear Lambert law

Photochemistry & Beer-Lambert`s Law | Physical Chemistry

Photochemistry & Beer-Lambert`s Law | Physical Chemistry

 i.e.  Photochemistry & Beer-Lambert`s Law | Physical Chemistry

Photochemistry & Beer-Lambert`s Law | Physical Chemistry

2 × 0.3010 = 0.5 ∈
∈ = 1.204 dm3 mol–1 cm–1

 

Q.2. A substance when dissolved in water at 10–3 M concentration absorbs 10 percent of incident radiation in a path of 1 cm length.  What should be the concentration of the solution in order to absorb go percent of the same solution?
 Sol.
∵ 10% absorbed then 90% transmitted
then     T =  Photochemistry & Beer-Lambert`s Law | Physical Chemistry= 90%

Photochemistry & Beer-Lambert`s Law | Physical Chemistry
Photochemistry & Beer-Lambert`s Law | Physical Chemistry…(1)

∵ 90% absorbed then 10% transmitted
then  Photochemistry & Beer-Lambert`s Law | Physical Chemistry

Photochemistry & Beer-Lambert`s Law | Physical Chemistry…(2)

Photochemistry & Beer-Lambert`s Law | Physical Chemistry
Photochemistry & Beer-Lambert`s Law | Physical Chemistry
Photochemistry & Beer-Lambert`s Law | Physical Chemistry

C = 0.0218 mol dm–3.


Q.3. In carbon-dating application of radioisotopes, 14C emits 
(1) β-particle (2) α-particle (3) γ--particle (4) positron 

Sol.  Photochemistry & Beer-Lambert`s Law | Physical Chemistry

Correct answer is (1)


Q.4. With the increase in temperature, Gibb’s free energy for the adsorption of a gas on a solid surface.
 (1) Becomes more positive from a positive value
 (2) Becomes more negative from a positive
 (3) Becomes more positive from a negative value
 (4) Becomes more negative from a negative value

Sol.  From Langmuir isotherm, the fractional coverage is
Photochemistry & Beer-Lambert`s Law | Physical Chemistry
∵ P ∝ T
Then higher the pressure or temperature lower the value of fractional coverage q.
R(g) + M(surface)  Photochemistry & Beer-Lambert`s Law | Physical Chemistry RM (surface)

if q decreases then the formation of RM decreases. i.e. rate of formation of RM decreases.
This indicates that Gibbs from the energy of adsorption becomes positive.
So, increase the temperature, the Gibbs free energy of adsorption of a gas on a solid surface become more positive from a negative value.
The correct answer is (3).

 

Q.5. One of the assumptions made in the conventional activated complex theory is:
 (1) Equilibrium is maintained between the reactants and the activated
 (2) Equilibrium is maintained between the reactants and the product
 (3) Equilibrium is maintained between the products and the activated complex
 (4) Equilibrium is maintained between the reactants, the activated complex and the products
 Sol.
  According to Eyring, the equilibrium is maintained between reactants and the activated complex

Photochemistry & Beer-Lambert`s Law | Physical Chemistry

(AB)# is the activated complex.
The correct answer is (1)


Q.6. For a reaction, the rate constant k at 27°C was found to be k = 5.4 × 1011 e–50 The activation energy of the reaction is
 (1) 50 J mol–1 (2) 415 J mol–1 (3) 15000 J mol–1 (4) 125000 J mol–1 

Sol.  From Arrhenius equation

k = Ae-Ea / RT &(1)
&
k = 5.4 × 1011 e–50 …(2)

From equation (1) & (2) we get

Photochemistry & Beer-Lambert`s Law | Physical Chemistry
Photochemistry & Beer-Lambert`s Law | Physical Chemistry

The correct answer is (4)

The document Photochemistry & Beer-Lambert's Law | Physical Chemistry is a part of the Chemistry Course Physical Chemistry.
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FAQs on Photochemistry & Beer-Lambert's Law - Physical Chemistry

1. What is the Beer-Lambert Law and how is it used in photochemistry?
Ans. The Beer-Lambert Law is a relationship that describes the attenuation of light as it passes through a medium. In photochemistry, it is used to quantify the absorption of light by a chemical species, which is essential for determining the concentration of the species in a solution.
2. How can the Beer-Lambert Law be applied to measure the concentration of a sample in photochemistry experiments?
Ans. In photochemistry experiments, the absorbance of a sample at a specific wavelength is measured using a spectrophotometer. By applying the Beer-Lambert Law, the concentration of the sample can be calculated by comparing the absorbance to a standard curve or using the formula A = εlc, where A is absorbance, ε is the molar absorptivity, l is the path length, and c is the concentration.
3. What are the limitations of the Beer-Lambert Law in photochemistry?
Ans. The Beer-Lambert Law assumes that the sample is homogeneous, the absorbing species are not interacting with each other, and the light source is monochromatic. In reality, these assumptions may not always hold true, leading to potential inaccuracies in concentration measurements.
4. How does the Beer-Lambert Law help in studying the kinetics of photochemical reactions?
Ans. The Beer-Lambert Law is used to monitor the change in concentration of reactants or products during a photochemical reaction. By measuring the absorbance at different time points, the rate of the reaction can be determined and kinetic parameters such as rate constants can be calculated.
5. Can the Beer-Lambert Law be used to determine the quantum yield of a photochemical reaction?
Ans. Yes, the Beer-Lambert Law can be used in conjunction with other experimental techniques to determine the quantum yield of a photochemical reaction. By measuring the absorbance and monitoring the conversion of reactants to products, the efficiency of the reaction in converting absorbed photons into chemical products can be calculated.
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