Consider a reaction taking place in an aqueous solvent. The transition state for this reaction is capable of interacting more strongly with the aqueous solvent (through low potential energy interactions, including hydrogen-bonding) than with the reactant/ground state. Despite these strong potential energy interactions, the reaction rate is not significantly faster than the same reaction taking place in a non-polar solvent. Why? a)The transition enthalpy is unchanged by the aqueous solvent b)The transition Gibbs energy is reduced in the aqueous solvent c) The transition entropy is significantly negative in the aqueous solvated reaction d) The transition state internal energy is significantly negative in the aqueous solvated reaction d) none of the above
Catalysis and Enzymatic Reactions
Catalysis is the kind of chemical reaction in which the rate (speed) of a reaction is enhanced by the catalyst which is not consumed during the process of reaction and afterward it is removed when the catalyst is not used to make up the impurity in the product. The enzymatic reaction is the reaction that is catalyzed via enzymes.
Lock And Key Model
The lock-and-key model is used to describe the catalytic enzyme activity, based on the interaction between enzyme and substrate. This model considers the lock as an enzyme and the key as a substrate to explain this model. The concept of how a unique distinct key only can have the access to open a particular lock resembles how the specific substrate can only fit into the particular active site of the enzyme. This is significant in understanding the intermolecular interaction between proteins and plays a vital role in drug interaction.
Consider a reaction taking place in an aqueous solvent. The transition state for this reaction is capable of interacting more strongly with the aqueous solvent (through low potential energy interactions, including hydrogen-bonding) than with the reactant/ground state. Despite these strong potential energy interactions, the reaction rate is not significantly faster than the same reaction taking place in a non-polar solvent. Why?
a)The transition enthalpy is unchanged by the aqueous solvent
b)The transition Gibbs energy is reduced in the aqueous solvent
c) The transition entropy is significantly negative in the aqueous solvated reaction
d) The transition state internal energy is significantly negative in the aqueous solvated reaction
d) none of the above
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