A 100% 7:07 PM Wed Feb 5 3 ... Unanswered •1 attempt left Rate law of a reaction is experimentally determined as Rate = k [A]^2 [B] The unit of k is 1/(M^2-sec) 1/(M-sec) sec/M M/sec M^2/sec Submit
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Q: A 100% 7:07 PM Wed Feb 5 Unanswered •1 attempt left For reaction 2A + 3B → 2C + D, following data of…
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- Examine the experimental data shown in the table below for the following reaction: (make sure to show your work for each part) A + 5B + 6C ---> 3D + 3E Experiment [A] (M) [B] (M) [C] (M) Rate (M/s) 1 0.35 0.35 0.35 8.0 x 10-4 2 0.70 0.35 0.35 3.2 x 10-3 3 0.70 0.70 0.35 6.4 x 10-3 4 0.70 0.35 0.70 3.2 x 10-3 A. What is the reaction order of A? B. What is the reaction order of B? C. What is the overall rate equation for this reaction? D. What is the value of the rate constant? E. What are the units of the rate constant?A general reaction written as A + 2B ® C + 2D is studied and yields the following data: [A]0 [B]0 Initial D[C]/Dt 0.150 M 0.150 M 8.00 ´ 10-3 mol/L·s 0.150 M 0.300 M 1.60 ´ 10-2 mol/L·s 0.300 M 0.150 M 3.20 ´ 10-2 mol/L·s Determine the initial rate of consumption ([deltaB]/delta t) for the first trial:For the reaction 2N2O5(g) → 4NO2(g) + O2(g), the following data were collected. t (minutes) [N2O5] (mol/L) 0 1.24 × 10–2 10. 0.92 × 10–2 20. 0.68 × 10–2 30. 0.50 × 10–2 40. 0.37 × 10–2 50. 0.28 × 10–2 70. 0.15 × 10–2 The concentration of O2 at t = 10. min is Question 16 options: A) 0.32 × 10–2 mol/L B) 2.0 × 10–4 mol/L C) 0.64 × 10–2 mol/L D) 0.16 × 10–2 mol/L E) none of these
- Reaction of interest : S2O82-(aq) + 3I- (aq)→ 2SO42-(aq) + I3-(aq). rate= k[S2O82-]1[I-]1.Consider the reaction Mn+ + ne- ⇌ M. If ΔG*c = ΔG* + (1-α)nFE and η = E – Eeq, prove that ic = io exp[-(1-α)nFηa)/RT)].Consider the reaction A(g) + 2B(g) → 2C(g) + 2D(g) and associated that was collected at a constant temperature. Trial Initial [A] Initial [B] Initial Rate (mol/L) (mol/L) (mol/(L·min)) 1 0.125 0.200 7.25 2 0.375 0.200 21.75 3 0.250 0.400 14.50 4 0.375 0.400 21.75
- Consider the base hydrolysis of an ester.RCOOR' + OH− → RCOO− + R'OH (where R and R' represent organic groups).The kinetics of this reaction, for a particular ester, were studied using the isolation method. When [OH−] << [RCOOR'] a pseudo-rate law can be posed:-d[OH-] / dt = k'' [OH-]mWith initial concentrations: [OH−]0 = 0.0015 M [RCOOR']0 = 0.700 M a plot of ln[OH-] versus t gave a straight line with slope = -0.0176 s-1 and y-intercept = -6.50.What is the order "m"?m = ? What is the corresponding pseudo rate constant k''? (include appropriate units)k'' = ?Given that :- Reaction => A + 2B ---> products Exp. Intial concentration [A] (mol/L) intial concentration [B] (mol/L) intial rate (mol/Ls) 1 0.115 0.135 2.70 × 10-3 2 0.115 0.270 2.16 × 10-2 3 0.345 0.135 8.10 × 10-3 What is the order of the reaction with respect to A, with respect to B, and overall?Initial temp: 19.06 C 0.5 M concentration 200 mL of HCl and 200 mL of NaOH are combined in an insulated container. H+(aq) + OH-(aq) - - -> H2O (l) ∆H H++ = 0, ∆H OH−− = -230 kJ/mol, ∆H H2O = -286 kJ/mol ∆H reactants = ∆H H++ + ∆H OH−− = -230 + 0 = -230 kJ/mol ∆H reactants = -286 kJ/mol - ( -230 kJ/mol) = -56 kJ/mol H+ (aq) + OH− (aq) - - -> H2O (l) Using your observations and the stoichiometric relationships of the reaction, determine the number of moles that react. Show/upload your work.
- For the following reaction 6 experiments have been run and the data collected is in the following table: 2 MnO4-(aq) + 5 H2C2O4 (aq) + 6 H+ (aq) ---> 2 Mn2+ (aq) + 10 CO2 (g) + 8 H2O (l) Experiment [MnO4-], M [H2C2O4], M [H+], M Rate, M/s 1 0.2410 0.3470 0.2690 0.1147 2 0.3260 0.6210 0.2270 0.2776 3 0.5630 0.5740 0.7420 0.4431 4 0.2410 0.3470 0.3840 0.1147 5 0.4140 0.5740 0.5610 0.3258 6 0.3260 0.4930 0.4910 0.2203 a) Find the order of the reaction with respect to H+. _______________ b) Find the order of the reaction with respect to MnO4-. ______________ c) Find the order of the reaction with respect to H2C2O4. _____________ d) What is the overall order of the reaction? ________________________The following reaction is carried out with [PCl5]i = 0.400 M at 25°C (i means initial) The reaction: PCl5(g)⇌PCl3(g)+Cl2(g) K= 0.00105 Using the small x approximation and "test x", could you please find the percent to two decimal places when testing x? Thank you so much.The data below was collected from three trials of the following reaction: 2ClO2 (aq) + 2OH- (aq) --> ClO3- (aq) + ClO2- (g) + H2O (l) [ClO2]o (M) [OH-]o (M) Initial Rate (M/s) 1 0.0500 0.100 5.75 x 10-2 2 0.100 0.100 2.30 x 10-1 3 0.100 0.0500 1.15 x 10-1 If the initial concentrations were as follows, [ClO2]o= 0.25 M and [OH- ]o = 0.095 M, what would the initial rate be?