Kinetics: Lindemann Mechanism Derivation

The video tutorial covers the Lindeman mechanism in physical chemistry, focusing on the derivation of the rate law using steady state approximation. It explains the role of intermediates and the assumptions that can simplify the reaction order. The tutorial also discusses how different assumptions about rate constants affect the apparent order of the reaction.

What is the primary concept used in the derivation of the Lindeman mechanism?

• Equilibrium constant

• Reaction quotient

• Le Chatelier's principle

• Steady state approximation

In the Lindeman mechanism, what does the 'A*' represent?

• A catalyst

• An activated intermediate

• A product of the reaction

• A reactant in its ground state

How is the concentration of the intermediate 'A*' expressed in terms of rate constants and reactants?

• K1 * A / (K2 * M + K-1)

• K2 * A / (K1 * M + K-1)

• K2 * A * M / (K1 * M + K-1)

• K1 * A * M / (K-1 * M + K2)

What happens to the reaction order if K-1 is much larger than K2?

• The reaction becomes second order with respect to A

• The reaction becomes first order with respect to A

• The reaction becomes first order with respect to M

• The reaction becomes zero order

If K2 is significantly larger than K-1, what is the apparent order of the reaction?

• Zero order

• First order with respect to A

• Second order overall

• First order with respect to M

Which assumption allows the simplification of the rate law to depend only on the concentration of A?

• K-1 is equal to K2

• K1 is equal to K2

• K-1 is much larger than K2

• K2 is much larger than K-1

What is the effect of assuming K2 is much larger than K-1 on the reaction order?

• The reaction becomes second order overall

• The reaction becomes first order with respect to A

• The reaction becomes first order with respect to M

• The reaction becomes zero order