For enzyme-catalyzed reactions that follow the mechanism $$\mathbf{E}+\mathbf{S} \rightleftharpoons \mathbf{E} \cdot \mathbf{S}$$ $$\mathrm{E} \cdot \mathrm{S} \rightleftharpoons \mathrm{E}+\mathrm{P}$$ a graph of the rate as a function of \([\mathrm{S}]\), the concentration of the substrate, has the following appearance: Note that at higher substrate concentrations the rate no longer changes with [S]. Suggest a reason for this.

Short Answer

Expert verified
At higher substrate concentrations, the rate of the enzyme-catalyzed reaction no longer changes with [S] because the enzyme molecules are saturated with the substrate. In this situation, all enzyme molecules are occupied with substrate and forming enzyme-substrate complexes. Adding more substrate does not result in any increase in the reaction rate since there are no unoccupied enzyme molecules available for additional substrates to interact with.

Step by step solution

01

Understand the reaction mechanism

First, we need to understand the reaction mechanism. The enzyme (E) interacts with the substrate (S) to form an enzyme-substrate complex (E·S). This step is reversible, meaning the complex can either dissociate back into enzyme and substrate or proceed to the second step. In the second step, the enzyme-substrate complex (E·S) breaks down into enzyme (E) and product (P). This step is also reversible. The rate of the enzyme-catalyzed reaction depends on the concentration of the substrate [S].
02

Investigate the enzyme saturation

At low substrate concentrations, the reaction rate increases as the substrate concentration increases. This is because there are more substrate molecules available for the enzymes to interact with, increasing the probability of the enzyme-substrate complex forming. However, at higher substrate concentrations, the rate no longer changes with [S]. This is because in high concentration of substrate, most enzyme molecules have already formed complexes with substrate molecules. This means that the enzyme is saturated, and the enzymes cannot take up any additional substrate molecules to react.
03

Understand the reason behind the constant reaction rate

As we increase [S], there is a point where the enzymes are working at their maximum capacity and cannot work any faster. This plateauing of reaction rate is due to the saturation of enzyme with the substrate. Since all the enzyme molecules are occupied with substrate and forming enzyme-substrate complexes, adding more substrate does not result in any increase in the reaction rate because there are no free enzyme molecules available for additional substrates to interact with. To conclude, at higher substrate concentrations, the rate of the enzyme-catalyzed reaction no longer changes with [S] because the enzyme molecules are saturated with the substrate, and further increases in substrate concentration does not result in any increase in the reaction rate.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Consider the reaction $$4 \mathrm{PH}_{3}(g) \longrightarrow \mathrm{P}_{4}(g)+6 \mathrm{H}_{2}(g)$$ If, in a certain experiment, over a specific time period, 0.0048 mole of \(\mathrm{PH}_{3}\) is consumed in a 2.0 - \(\mathrm{L}\) container each second of reaction, what are the rates of production of \(\mathbf{P}_{4}\) and \(\mathbf{H}_{2}\) in this experiment?

A reaction of the form $$aA \longrightarrow Products$$gives a plot of \(\ln [\mathrm{A}]\) versus time (in seconds), which is a straight line with a slope of \(-7.35 \times 10^{-3} .\) Assuming \([\mathrm{A}]_{0}=\) \(0.0100 M,\) calculate the time (in seconds) required for the reaction to reach \(22.9 \%\) completion.

The activation energy of a certain uncatalyzed biochemical reaction is \(50.0 \space\mathrm{kJ} / \mathrm{mol} .\) In the presence of a catalyst at \(37^{\circ} \mathrm{C}\) the rate constant for the reaction increases by a factor of \(2.50 \times 10^{3}\) as compared with the uncatalyzed reaction. Assuming the frequency factor \(A\) is the same for both the catalyzed and uncatalyzed reactions, calculate the activation energy for the catalyzed reaction.

Chemists commonly use a rule of thumb that an increase of \(10 \space\mathrm{K}\) in temperature doubles the rate of a reaction. What must the activation energy be for this statement to be true for a temperature increase from 25 to \(35^{\circ} \mathrm{C} ?\)

A reaction of the form $$aA \longrightarrow Products$$gives a plot of \(\ln [\mathrm{A}]\) versus time (in seconds), which is a straight line with a slope of \(-7.35 \times 10^{-3} .\) Assuming \([\mathrm{A}]_{0}=\) \(0.0100 M,\) calculate the time (in seconds) required for the reaction to reach \(22.9 \%\) completion.

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free