5. Consider the reaction below. If the reaction is uncatalyzed k=10's', if it is catalyzed k₁ = 10's'. For the uncatalyzed reaction k=10³s¹. k₁ k₁ a) What is K for the uncatalyzed reaction? cq b) Does it change for the catalyzed reaction? Why or why not? 5. If the middle line (darker one) is the rate of an enzyme reaction in the presence of an uncompetitive inhibitor, which line number represents the reaction without the inhibitor? Explain your answer. [S] 7. Draw a Lineweaver-Burk plot of the graph in the previous question. Values are not necessary just comparative shapes of lines. (Label axis and y intercept)

5. Consider the reaction below. If the reaction is uncatalyzed k=10's', if it is catalyzed k₁ = 10's'. For the uncatalyzed reaction k=10³s¹. k₁ k₁ a) What is K for the uncatalyzed reaction? cq b) Does it change for the catalyzed reaction? Why or why not? 5. If the middle line (darker one) is the rate of an enzyme reaction in the presence of an uncompetitive inhibitor, which line number represents the reaction without the inhibitor? Explain your answer. [S] 7. Draw a Lineweaver-Burk plot of the graph in the previous question. Values are not necessary just comparative shapes of lines. (Label axis and y intercept)

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

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Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
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11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
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. Account for the increase in reaction rate brought about by a catalyst.
The rate of a certain reaction doubles for every 10 C rise in temperature. (a) How much faster does the reaction proceed at 45 C than at 25 C? (b) How much faster does the reaction proceed at 95 C than at 25 C?