ucose-cocp-2000+100g ge Find Cyoy the value of the [HgCl2] (M) [C2042-1 (M) | Rate (Mis) 0.10 0.10 1.3.10-7 0.10 0.20 5.2.10-7 0.20 0.20 1.0-10-6 A) 1.4 x 10-8 1/M2-s B) 1.3 x 10-7 1/M2-s C) 1.4 x 10-5 1/M2-s D) 1.3 × 10-4 1/M2-s
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- Reaction Velocity (mm/sec) Ma no !! L [1 1 L IM 3M FO Substrate Concentration (M) 1. IN Which statement is true? KM AN ALM 4V The graph above displays the kinetic profiles of the same enzyme catalyzing two different substrates. The red curve displays the higher turnover number (kcat). The red curve displays higher affinity between substrate and enzyme. The blue curve displays competitive inhibition. The red curve displays higher cooperativity,2 HgCl2 + C204²-→2 Cl* + Hg2Cl2 + 2 CO2 Initial Rate, M Experiment [HgCl]o, M [C2042-]o, M 1 S 1 0.365 0.446 6.85x10-4 0.730 0.446 1.37×10-3 3 0.365 0.891 2.74x10-3 4 0.730 0.891 5.47x10-3 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M-2s-1.The following initial rate data were obtained on the rate of binding of glucose with the enzyme hexokinase (from yeast) present at a concentration of 1.34 mmol/dm3. [C6H12O6] / (mmol dm-3) 1.00 1.54 3.12 4.02 Initial speed v0 / (mol dm-3 s-1) 5.00 7.60 15.5 20.0 use the data above to calculate the rate constant. k = ________ (mol/L/s, s-1, L/mol/s, or L2/mol2/s). 3 s.f. normal format.
- The following initial rate data were obtained on the rate of binding of glucose with the enzyme hexokinase (from yeast) present at a concentration of 1.34 mmol/dm3. [C6H12O6] / (mmol dm-3) 1.00 1.54 3.12 4.02 Initial speed v0 / (mol dm-3 s-1) 5.00 7.60 15.5 20.0 (a) What is the order of the reaction with respect to glucose? (b) use the data above to calculate the rate constant. k = ________ (mol/L/s, s-1, L/mol/s, or L2/mol2/s). 3 s.f. normal formatNH4+ {aq) + NO2(aq) -> N2(g) +2H2O{l} Data Initial [NH4+] Initial [NO2-] rate 1 0.0100 0.200 5.4 x10-7 2 0.0200 0.200 10.8x10-7 3 0.0400 0.200 21.5x10-7 4 0.200 0.0202 10.8x10-7 5 0.200 0.0404 21.6x10-7 6 0.200 0.0808 43.3x10-7 Find x,y,kPERTINENT CALCULATIONS Remember: rate = k[C25H30CIN3]"[OH_]" where n =0 since excess OH was used. n3= 1. Refer to your graphs and complete table below Linear correlation (r- value) Graph Kinetic Run I Kinetic Run II Average r- value absorbance vs time 0.9972 0.9955 0.9964 In (absorbance) vs time 0.9978 0.9994 0.9986 2/(absorbance) vs time 0.9805 0.9879 0.9952 2. Based on the average linear correlation (r2 -value) the reaction order, m, with respect to crystal violet, CV, is Explain. 3. Write the rate law. 4. The slope, and therefore pseudo" rate constant, kr', is at T1. CC, and ko' is at T2
- The following data were obtained in a study of an enzyme known to follow Michaelis-Menten kinetics. Product formed (mmol/min) Substrate added (mmol/L) 217 0.8 325 2 433 4 488 6 647 1000 The Km for this enzyme is approximately: 4 mM. 2 mM. 1 mM. 6 mM. 1000 mM.5. What is the value for the rate constant, k? k = k'/1* = k = k"/0.5* = kavg r = k[OH°]*[ C25H3„N,'J" [OH] C2H,„N;'] r = 3034) The rate of the following rxn depends only on NO₂: NO₂ + CO NO + CO₂. The following data was collected from a kinetics experiment: Time (s) 0 1200. 3000. 4500. 9000. 18000. [NO₂] (mol/L) 0.500 0.444 0.381 0.340 0.250 -0.174 1 I a. Order with respect to NO₂: the best R2 value in order to find the rate of the reaction) (Ans: 2nd order-r' value of 0.999) b. Rate law for this reaction: (Hint: [NO₂]. Ln[NO₂] and 1/[NO₂] and find (Ans: rate= K[NO₂] ²) c. [NO₂] at 2.7 x 104 s after the start of the rxn: 2nd order reaction rate law) (Hint: use the integrated
- Question 10 of 11 Submit What is the activation energy for the isomerization of methyl isocyanide? Rate Constant Temperature 4.30 x 10-3 min-1 472 K 5.54 x 10-2 min-1 503 K kJ/mol 1 2 3 4 6. C 7 8 +/- x 10 0 Tap here or pull up for additional resources LOThe reaction mechanism shown below includes which of the catalytic mechanism types (Choose all that apply) Mg?+ PO?- Mg2+ PO? O H он Mg2+ -Ċ-H Mg2 -C-H H ÓH OH нон H-N-H "HO H-N-H H. Lys345 Lys345 Glu211 O transition state stabilization binding catalysis O metal ion catalysis O covalent catalysis O acid catalysis electrostatic catalysis O proximity binding catalysis O base catalysis O electron sink displacement catalysisA+B+CD Exp. Initial A (mol/dm³) Initial B (mol/dm³) Init. Rate of Formation of D (mol/dm³ min-¹) 1 0.10 0.10 3.0 x 10-4 2 0.30 0.30 9.0 x 10-4 3 0.10 0.30 3.0 x 10-4 4 0.20 0.40 6.0 x 10-4 5 0.10 0.10 1.2 x 10-3 The student concluded that the rate equation should be: rate = K[A] [B][C]² ii) Using the data for experiment 4, calculate the value of the rate constant, k, using the correct rate equation, making sure that you include the correct units. Initial C (mol/dm³) 0.10 0.10 0.10 0.10 0.20