plz give answer correctly in detail 2. Consider an uncatalyzed reaction: SPwhere k, = 100 s-¹ and k₁ = 1 s¹¹. Now, consider the same reaction catalyzed by an enzyme in whichk₁ = 1,000,000 s1. What is k, in the enzyme-catalyzed reaction?A. Depends on whether the reaction is just starting or has reached equilibrium.B. 1 s1C. 1000 s¹D. 10,000 s¹E. 100,000 s¹

Answered: Image /qna-images/answer/bf402cc6-376f-412f-89e2-466915de8a11.jpg

2. Consider an uncatalyzed reaction: S P where k, = 100 s-¹ and k₁ = 1 s¹. Now, consider the same reaction catalyzed by an enzyme in which k₁ = 1,000,000 s¹¹. What is k, in the enzyme-catalyzed reaction? A. Depends on whether the reaction is just starting or has reached equilibrium. B. 1 s¹ C. 1000 s1 D. 10,000 s¹ E. 100,000 s¹¹

2. Consider an uncatalyzed reaction: S P where k, = 100 s-¹ and k₁ = 1 s¹. Now, consider the same reaction catalyzed by an enzyme in which k₁ = 1,000,000 s¹¹. What is k, in the enzyme-catalyzed reaction? A. Depends on whether the reaction is just starting or has reached equilibrium. B. 1 s¹ C. 1000 s1 D. 10,000 s¹ E. 100,000 s¹¹

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 26Q: Consider the following relationships: G = 1, H = TS, Q = 1. G = G, K = 1 Which of these...

See similar textbooks

Similar questions

a. Using the free energy profile for a simple one-step reaction, show that at equilibrium K = kf/kr, where kf and kr, are the rate constants for the forward and reverse reactions. Hint: Use the relationship G = RT ln(K) and represent kf and kr, using the Arrhenius equation.(K=AeEa/RT) b. Why is the following statement false? A catalyst can increase the rate of a forward reaction but not the rote of the reverse reaction.
Why are there no changes specified for Ni in Exercise 13.61, part (f)? What property of Ni does change?
. Suppose a reaction has the equilibrium constant K=1.7108at a particular temperature. Will there be a large or small amount of unreacted starting material present when this reaction reaches equilibrium? Is this reaction likely to be a good source of products at this temperature?
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
At 25C. Kp 1 1031 for the reaction a. Calculate the concentration of NO, in molecules/cm3, that can exist in equilibrium in air at 25C. In air, PN2=0.8 atm and PO2=0.2atm. b. Typical concentrations of NO in relatively pristine environments range from 108 to 1010 molecules/cm3 Why is there a discrepancy between these values and your answer to part a?
What are homogeneous equilibria? Heterogeneous equilibria? What is the difference in writing K expressions for homogeneous versus heterogeneous reactions? Summarize which species are included in the K expression and which species are not included.
Consider the following relationships: G = 1, H = TS, Q = 1. G = G, K = 1 Which of these relationships is(are) always true for a reaction at equilibrium?
In Chapter 3, we discussed the conversion of biomass into biofuels. One important area of research associated with biofuels is the identification and development of suitable catalysts to increase the rate at which fuels can be produced. Do a web search to find an article describing biofuel catalysts. Then, write one or two sentences describing the reactions being catalyzed, and identify the catalyst as homogeneous or heterogeneous.
In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.
Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the interconversion reaction?
. At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide. N2(g)+O2(g)2NO(g)Suppose the system is analyzed at a particular temperature, and the equilibrium concentrations arc found to be [N2]=0.041M. [O2]=0.0078M, and [NO]=4.710M. Calculate the value of K for the reaction.