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- Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.0 State what rate law you would expect from this mechanism (Rate = k[Acetone]"[H*]"[[₂]') • Compare the expected rate law from the mechanism to the rate law you got from the Method of Initial rates and the Method of Isolation. If they are different, suggest 1-2 valid, specific, experimental reasons why they might be different. (fast, equilibrium) CH3 ソース H3C ག་ CH3 + H* = H3C H3C H. + H (slow) CH3 H3C CH2 + ↳2 Т + HI3. The following reaction: A' (a) + B (ag + C (an)→ G* (ae) +2 H ) AH = -250 kJ There are two proposed mechanism: Mechanism 1 A' () + B aa) AB' a) + D (a) Step 1 AB" (a) (fast) + E (a) + Hm → G' sae) + H ) + D² (n) Step 2 (slow) Step 3 E (agi+ C (a) (fast) Mechanism 2: Step 1 AB' (a) A' (an) + B (ag) AB' (a) + C ja) (fast) Step 2 + G' (a) + 2 H() (slow) The reactions was determined to have the following rate law: r= k[A'][B] a) Which of the two proposed mechanisms is valid? Explain. b) List any reaction intermediates: catalysts: c) What is a rate determining step? d) If the activation energy for the overall forward reaction is 150 kJ, sketch the potential energy diagram for the above reaction; showing the overall reaction, the reaction mechanism, labelling the AHu, AHy, Eapu, Eag, reaction intermediates, and activated complex. rvs fwd drvs/
- Given the following reaction CH3NNCH3(g) ==> C2H6(g) + N2(g) and the measured kinetic data below: [ CH3NNCH3(g) ] M Rate M/s 0.0113 2.86 x 10-6 0.0226 1.28 x 10-5 what is the order with respect to (each of the) reactants CH3NNCH3(g),? Type your calculated answer for CH3NNCH3(g) here:1:35 PM Sun Jan 30 *2 30% ID < 88 Q CHM1046 Ch 19 Kinetics v x PSY 2012 Ch 1 Guiding Q - Cra.. Calorimetry Quiz CHM 1046 TLC CHM1046 Ch 19 Kinetics y Equations 1) The isomerization reaction shown below follows first order kinetics at 500 K. CH3NC (g) → CH3CN (g) a) Use the rate constant you determined in example 3 on page 4 to determine the half life of this reaction. K? 6. 579 x 10 half ll fe 0.693 6. S19 x 10-9 16 S3 . 35 %3D b) Use the half life you just determined to predit how long it will take for the concentration of CH3NC to reach 25% of its original value? 28 of 44bel the energy diagram (9 bins) for the conversion shown. H₂O (CH₂CH₂), CBr - 000 000 F4 % 5 T G exergy F5 6 (CH₂CH₂)3COH + H₂O*Br Y H reaction coordinate MacBook Pro & 7 U F7 J = * 0 8 DII F8 1 K ( 9 DD O O L activation energy Answer Bank products F10 rate-limiting transition state non-limiting transition state intermediates P starting materials F11 { AG° + 11 F12 11 )
- /5 C12-3-09 Explain the concept of a reaction mechanism. Include: rate-determining step 4. What is a reaction mechanism? 5. Why is a bimolecular step more reasonable than a termolecular step? 6. Considerthe following mechanism: Step 1: ClO (aq) + H2O) → HCIO(aq) + OH'(aq) [Slow] Step 2: l'(aq) + HCIO aq) → HIO(aq) + Cl a« (aq) [Fast] Step 3: OH (ag) + HIO(aq) → H2O +10 (aq) [Fast] a. What is the overall equation? b. Identify any intermediates С. What is the rate determining step? Why did you choose this step? d. In which step is the catalyst placed? Why is it put in this step? e. Predict and explain the effect the following changes would have on the rate of the reaction. 7 lowe,t i. Increasing the concentration of Clo- ii. Increasing the concentration of I for frst6) Draw an energy profile diagram with AH = -10 kJ and E₂ (Activation Energy) = +25 kJ. Label: reactants, products, transition state, and values on the y-axis to verify the values of AH and E. - 101 Frient of practionThe following mechanism has been proposed for the reaction: C,H5COOH = CH;CO,H; fast; constants k,and k_1) C,HsCO2H e CgH5CO* + H20 (fast, constants kɔand k-2) C,H;CO + HX + H20 C,H,NH, + N2 + CO2 (slow; constant k,) A. What intermediate(s) are formed in this mechanism? B. What is the rate law, based on the above mechanism? C. The overall rate constant for this reaction is 0.200 x 10 L mol's. Is this value consistent with your answer to B? Explain. D. Sketch a reaction-energy diagram consistent with the above mechanism and the enthalpy change calculated earlier. Label the enthalpy change and each transition state. Explain the appearance of your graph.
- 1. A → B +B (rate constant = k1) 2. A +B → C+D (rate constant = k2 3. D → E+F (rate constant = k3) 4. F+A → D + G (rate constant = k Express the net change of [F] and [G]& (select 2 answers) а. d[F] = -k3[D]+k4[A][F] dt b. d[G] = -k4[A][F] dt d[E] = -k3[D] dt d[F] = k3[D]-k4[A][F] С. dt d. d[F] = k3[E][F]-k4[A][F] dt = k4[A][F] dt е. d[E] = k3[D] dt f. d[G] = k4[D][G] %3D dt d[E] = k3[E][F] dt(Q80) Using the information provided (and your work from Q79), what is the numerical value of the rate constant for the rate law determined in Q79? CHCI3 (g) + Cl2 (g) --> CCI4 (g) + HCI (g) [CHCI3] (M) [C2] (M) Initial Rate (M/s) 0.010 0.010 0.0035 0.020 0.010 0.0069 0.020 0.020 0.0098 0.040 0.040 0.027The reaction H2O + SO3 → H2SO4 is a source of acid rain in Earth’s atmosphere. It is thought to occur via the two-step mechanism shown at the right. (1) H2O+SO3 -->H2OSO3 (2) H2O+H2OSO3-->H2O+H2SO4 a. What is the experimental rate law for the overall reaction if step (1) is the rate determining step? b. What is the experimental rate law for the overall reaction if step (2) is the rate determining step?
