Mechanism 1 Mechanism 2 Mechanism 3 10. Three different mechanisms are A+Y C+D slow B+C E+Y fast A → Q+D sk B+Q→ E A+B > F slow proposed for an exothermic reaction, shown here: → D+E fast F fa a)What is the overall reaction? (in box) b)Circle any intermediates(s) in these mechanisms. c)Put a box around any catalyst(s) in these mechanisms. d)Do any of these mechanisms have a second order rate law? If yes, circle here: Mech 1 Mech 2 Mech 3

Mechanism 1 Mechanism 2 Mechanism 3 10. Three different mechanisms are A+Y C+D slow B+C E+Y fast A → Q+D sk B+Q→ E A+B > F slow proposed for an exothermic reaction, shown here: → D+E fast F fa a)What is the overall reaction? (in box) b)Circle any intermediates(s) in these mechanisms. c)Put a box around any catalyst(s) in these mechanisms. d)Do any of these mechanisms have a second order rate law? If yes, circle here: Mech 1 Mech 2 Mech 3

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Use the following data to calculate the reaction rate law and the rate law constant for the system. ??(?)+?2(?)→???2(?) Trial Run [NO] (mol/L) [H2] (mol/L) Initial Rate (mol/L∙s) 1 0.001 0.004 0.002 2 0.002 0.004 0.008 3 . 0.003 0.004 0.018 4 0.004 0.001 0.008 5 0.004 0.002 0.016 6 . 0.004 0.003 0.024 a) rate = k[NO][H2]2, where k = 7 L2/mol2∙s b) rate = k[NO]2[H2], where k = 5.0x105 L2/mol2∙s c) rate = k[NO][H2], where k = 5.0x105 L2/mol∙s d) rate = k[NO]2[H2]3, where k = 3.0x10-7 L/mol2∙s
1 and 2
8) What was the change in reaction time? a) no change b) slower time = (faster time) x 2 c) slower time = (faster time) to the power of 2 d) there is no relationship between reaction times and concentration change
O b с a The activation energy diagram for the reaction A + B →→C + D is shown below. Which arrow represents the activation energy (E₂) of the reverse reaction? Energy A+B Extent of reaction Not enough information Transition state C+D
What is the order of the reaction A → B given the plot shown? 400 A) Zero 300 B) First 200 C) Second 100 D) Third E) Cannot determine order from this information 60 120 180 240 300 360 Time (s) నాజం Esc F7 F10 F11 F12 insest F6 FB F9 F3 F4 F5 FI % & డా %23 %3D 3 4 7 8 9 1/[A] (M-')
Considering the following diagram, the activation energy of the reverse reaction is about 160 120 80- Products 40 Reactants Reaction progress A) 60 kJ/mol B) 80 kJ/mol C) 130 kJ/mol D) 20 kJ/mol Energy (kJ/mol)
人工知能を使用せず、すべてを段階的にデジタル形式で解決してください。ありがとう SOLVE STEP BY STEP IN DIGITAL FORMAT DON'T USE CHATGPT 7.- Consider the following reaction energy diagram. Answer what is asked of you below: a) Label the reactants and products. Mark the activation energy of the first and second steps. b) Is the overall reaction endothermic or exothermic? What is the sign of the AH°? c) Point out the intermediates and transition states. d) Mark the transition state of the rate-limiting step.
A student proposes the following step of a mechanism. Why would an expert question this mechanism step? 3 A + B → 2 C A) The number of reactants and products must be the same. B) The number of products must always exceed the reactants. C) This would require 4 molecules to collide and react simultaneously. D) This step should be reversible. E) An expert would not question this step.
A: Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3- --> 4 Zn2+ + N2O(g) + 5 H2O(l) What is the rate of Zn2+ formation if its concentration rises from 0.00 to 0.069 M in 2 minutes and 12 seconds? Group of answer choices 0.031 M/s 2.1 x 10-3 M/s 1.3 x 10-4 M/s 5.2 x 10-4 M/s B: Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3- --> 4 Zn2+ + N2O(g) + 5 H2O(l) If the rate of H+ disappearance is 0.0250 M/min, what is the rate of Zn2+ appearance? Group of answer choices 0.0100 M/min 0.00100 M/min 0.0250 M/min 0.0625 M/min
E. For the reaction A+B+C→D+EA+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A][A](MM) [B][B](MM) [C][C](MM) Initial rate(M/sM/s) 1 0.30 0.30 0.30 9.0×10−5 2 0.30 0.30 0.90 2.7×10−4 3 0.60 0.30 0.30 3.6×10−4 4 0.60 0.60 0.30 3.6×10−4
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