The mechanism proposed for the oxidation of iodide ion by the hypochlorite ion is shown below. Step 1 Step 2 CIO + H₂O I + HCIO HIO + OH HCIO + OH → HIO + CI (fast, equilibrium) This is reversible Step 3 IO + H₂O (fast) This is not reversible a. What is the overall reaction for this mechanism? Answer within the test and not on scratch paper. b. What are the intermediates if any are present? Answer within the test and not on scratch paper. c. What is the rate law expression for each step of the mechanism (including any reversible steps)? Answer this question on your scratch paper, clearly labeled. d. What is the predicted rate law expression for this reaction? Show all work to receive any credit. Answer this on your scratch paper, clearly labeled e. What would be the expected units for k using seconds for the time unit? Answer within the test and not on the scratch paper. (slow) This is not reversible

A. Consider the reaction mechanism shown below Step 1. H₂O2 +J H₂O + 10. slow Step 2. IO + H2Oz H₂O + O2 + I fast What is the overall balanced chemical equation? Group of answer choices H₂O2 → H₂O + O2 2 H2O2 → 2 H₂O + O2 none of the answers are correct

What is true about the diagram? A.) The step from A->B is the slow step   because activation energy is high. B.) Step B-->C is the rate limiting step. C.) The reaction is endothermic. D.) There is one transition state showing. Please refer to the attached photo for the diagram.

Answer the following question using the reaction coordináte diagram shown below. 280 240 200 160 120- 80 40 Time What is the activation energy for the reverse reaction? O A. -160 kJ B. -80 kJ O C. 80 kJ D. 160 kJ tent (H) kilojoules

Consider this graph of concentration versus time. Concentration (M) V 1.00 0.84 0.52 0.32 0.00 1st attempt Part 1 X - + Time log B₂ A₂ A3B What is the mass action expression for the reaction? Do not add multiplication symbols or spaces to your answer. Feedback cos. 8 See Periodic Table See Hint

Energy Diagram Reaction Time (min) Which of the following statements is true for the graph shown above?- The prodrcts bave hioh 1. 1. Potential Energy (kJ)

Figure 1. Nitrite concentration versus time for the reaction of ammonium ion with nitrite. Tangent lines at t= 0 and 75,000 s indicated in red. nitrite concentration (M) NH4 (aq) + NO₂ (aq) N2(g) +2 H₂O(l) [NO₂ ]0=0.0050 M [NH4*]0=0.100 M 0.005 0.004- 0.003- 0.002- 0.001- t=0 s 50000 100000 Time (s) t = 75,000 s 150000 200000 Critical Thinking Questions 1. What is the instantaneous reaction rate at t= 0 seconds? 2. What is the instantaneous reaction rate at t= 75,000 seconds? 3. What is the average reaction rate over the first 30,000 second time interval? 4. What is the average reaction rate over the next 30,000 second time interval? 5. How does the rate of reaction change as [NO₂] decreases? 6. Estimate the instantaneous reaction rate at t = 200,000 seconds. Explain your reasoning.

Use the information provided in the table below to answer the next two questions. The reaction between reactants A and B was studied at-10 °C. The following results were obtained. Experiment Initial [A] (mol/L) Initial [B] (mol/L) Initial Reaction Rate (M/min) 1 0.10 0.10 0.18 0.10 0.20 0.36 3 0.20 0.20 1.45 11. What is the order with respect to [B]? (a) 1 (b) 2 (c) ½ (d) 0 12. What is the order with respect to [A]? (a) 1 (b) 2 (c) ½ (d) 0