ST6B3- Use the initial rate data below to determine the rate law for the decomposition of A into products. Report only the reaction order for A [involving M and s in some combination]. Note 1: The reaction order in this randomized problem will NOT be an integer. Note 2: The data table in the text for this problem is faulty; it will not yield the answers printed. Trial 1 Trial 2 [A]o (mM) vo (mM/s) 5.0 9.1 3.0 10.0 Type your answer.
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- Part B: Integrated rate law expressions for zero- and half-order reactionsDerive integrated rate law expressions for half-, one and a half-, and third-order reactions of the form A products where k is the rate constant. Also, deduce the graphical linear relations, units of rate constant k, and expression for half-life, t1/2 , for all cases. Assume that at t = 0 only A is present with an initial concentration of [A]0. Fill in the table below by following the example given for first-order reaction1.Explain the mechanism and potential energy surface of the reaction. N2O + hv → N2 + O Now choose an appropriate theory and describe how you would use it to determine the rate coefficient.Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.340 0.210 0.0204 2 0.340 0.420 0.0204 3 0.680 0.210 0.0816 ?=
- The following results were found after completion of Part C in the Experimental procedure: 0.056 M I- and 0.048 M H2O2 were used Run Catalyst Calculated Rate of Reaction (M/s) 1 none 0.031 2 10.00mL of 0.35 M FeCl2 0.52 Assuming the Rate Law = k[I-][H2O2] 2 Calculate the value of k for run 2. Give your answer to the nearest whole number.Using the data in the table, determine the rate constant of the reaction and select the appropriate units. A+2B⟶C+D Trial [?] (?) [?] (?) Rate (M/s) 1 0.360 0.290 0.0144 2 0.360 0.580 0.0144 3 0.720 0.290 0.0576 k=The recombination reaction2 HO2(g) → H2O2(g) + O2(g)has a second-order rate constant of 1.7E9 M-1 s-1. Calculate the half-life of the reaction if the initial concentration of HO2(g) is 2.22E-11 M.Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is:1/ct = 1/c0 + 2kt Give the answer to 3 significant figures
- 2H2O2(aq) --> 2H2O(l) + O2(g) rate expression: rate = k[H2O2]m[I-]n 1. a) What experimental factors change the numerical value of n in the rate law for the reaction of H2O2 with I-? b) What experimental factors change the numerical value of k in the rate law for the reaction of H2O2 with I-?In the experiment, below gas-phase homogenous oxidation, k 2 NO + O2 -------> 2NO2 was confirmed to have the third-order kinetics, showing an elementary reaction, at least for low partial pressures of nitrogen oxides. However, the rate constant k actually decreases with increasing absolute temperature, indicating an apparently negative activation energy. It is known that any elementary reaction must have a positive energy. Provide an explanation, starting from the fact that an active intermediate species, NO3, is a participant in some other know reactions that involve oxides of nitrogen. Other active intermediates could be NO* and O2* and O* (oxygen atom). Using chemical reactions, or reaction pathway, to describe the mechanism, and using your own reactions suggest how to postulate the formation rate of NO2.Consider the following 3 step reaction mechanism: Step 1 H2 2H fast Step 2 H + CO HCO slow Step 3 H + HCO H2CO fast 1). What is the overall reaction? 2). Identify the intermediates in the reaction mechanism. 3). Write a rate law expression for each step of the mechanism including any reversible reactions. 4). What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates in the rate law expression.
- A + 3B + 2C --> D + 2E Determine the rate law and rate constant using the experimental data below [A] (M) [B] (M) [C] (M) Rate (M/sec) Exp. 1 0.100 5.00 x 10-4 1.00 x 10-2 0.137 Exp. 2 0.100 1.00 x 10-3 1.00 x 10-2 0.268 Exp. 3 0.200 1.00 x 10-3 1.00 x 10-2 0.542 Exp. 4 0.400 1.00 x 10-3 2.00 x 10-2 1.084At 45 degrees Celsius, the N2O5 is monitored. Answer the data and determine the line's equation and R² and make the tables 3 and 4 are plotted in one graph. What is the slope of the line that is rate constant? Which model is the best?a) Briefly outline how you could determine the rate constant, k, of the reaction using this virtual experiment simulation. b) IO3- + 3 H3AsO3 → I- + 6 H+ + 3 HAsO42- . (Reaction 3) (catalysed by I-) This proceeds via two main reactions: 6 H+ + IO3- + 8 I- → 3 I3- + 3 H2O (Reaction 1) rate limiting step Followed by this rapid reaction: H3AsO3 + I3- + H2O → HAsO42- + 3 I- + 4 H+ (Reaction Over the course of the reaction (3), what would happen to the reaction rate if the pH was not maintained using acetic acid/sodium acetate buffers in the pH range 4 -5 but allowed to vary instead?