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Physisorption Chemisorption Forces of attraction are vander Waals' forces Forces of attraction are chemical bond forces Low enthalpy of adsorption (20 - 40 k.J/mole) High enthapy of adsorption (200 - 400 k.J/mole) This process is observed under conditions of low temperature This process takes place at high temperatures It is not specific It is highly specific Multi-molecular layers may be formed Generally, monomolecular layer is formed This process is reversible This process is irreversible
Physisorption involves weak van der Waals forces between the adsorbate and adsorbent, while non-activated chemisorption involves stronger chemical bonds forming between the two. Physisorption typically occurs at lower temperatures and can be easily reversed, while non-activated chemisorption requires higher temperatures and is more difficult to reverse.
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Why Physisorption is multilayered and chemisorption is monolayered?
physisorption involves van der wall attractive forces between adsorbent and adsorbed , This may result on the accumulation of many layers of the molecules on the surface. Chemosorption involves formation of chemical bonds between adsorbent and adsorbed molecule. Adsorbent have some functional groups or atoms on its surface with unsatisfied valences, once these valences are satisfied they don't undergo bond formation with more adsorbed molecules and only single layer is formed.
Why physisorption decreases with increase in temperature?
Physisorption involves weak van der Waals forces between gas molecules and a solid surface. As temperature increases, gas molecules gain more kinetic energy, making it harder for them to be retained on the surface through weak interactions. This leads to a decrease in physisorption at higher temperatures.
What is the difference between an activated complex and an intermediate?
An activated complex refers to the highest energy state along the reaction pathway, representing the transition state between reactants and products. An intermediate is a stable species formed during the reaction but is not the final product. It can be a product of one step and a reactant in the next step of the reaction.
What is the difference between activated charcoal and deactivated charcoal?
Activated charcoal is treated to have a large surface area for adsorption, making it effective for detoxification and filtration purposes. Deactivated charcoal, on the other hand, has a reduced adsorption capacity as it is not designed for active use in absorbing toxins or chemicals.
What is an activated complex?
An activated complex is an intermediate state in a chemical reaction where the reactant molecules are at their highest energy level before forming products. It represents a critical point in the reaction where old bonds are breaking and new bonds are forming.
Why is enthalpy of chemisorption higher than physisorption?
The enthalpy of chemisorption is higher than physisorption because chemisorption involves the formation of chemical bonds between the adsorbate and the adsorbent surface, which requires more energy to break than the weaker van der Waals forces involved in physisorption. This leads to a stronger interaction between the species adsorbed on the surface, resulting in a higher enthalpy of chemisorption.
Is adsorption of oxalic acid on charcoal physisorption or chemisorption?
The adsorption of oxalic acid on charcoal is typically considered to be physisorption. Physisorption involves weak van der Waals forces between the adsorbate (oxalic acid) molecules and the surface of the adsorbent (charcoal). Chemisorption, on the other hand, involves stronger chemical bonds and typically requires more energy.
Why does physisorption decrease with the increase of temperature?
Physisorption is weaker than chemisorption and is typically dependent on van der Waals forces. As temperature increases, the thermal energy disrupts these weak interactions between the adsorbate and the surface, leading to a decrease in physisorption.
Why Physisorption is multilayered and chemisorption is monolayered?
physisorption involves van der wall attractive forces between adsorbent and adsorbed , This may result on the accumulation of many layers of the molecules on the surface. Chemosorption involves formation of chemical bonds between adsorbent and adsorbed molecule. Adsorbent have some functional groups or atoms on its surface with unsatisfied valences, once these valences are satisfied they don't undergo bond formation with more adsorbed molecules and only single layer is formed.
Why physisorption decreases with increase in temperature?
Physisorption involves weak van der Waals forces between gas molecules and a solid surface. As temperature increases, gas molecules gain more kinetic energy, making it harder for them to be retained on the surface through weak interactions. This leads to a decrease in physisorption at higher temperatures.
Is physisorption a reversible process?
Yes, physisorption is generally considered a reversible process because it involves weak van der Waals forces or electrostatic interactions between the adsorbate molecules and the adsorbent surface. This means that the adsorbate molecules can easily desorb from the surface under suitable conditions, making physisorption reversible.
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What is the difference between an activated complex and an intermediate?
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