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- The following data was collected over five different experiments. for this reaction: BF3 + NH3 → F3BNH3 Experiment [BF3] M [NH3] M 1 0.250 0.250 2 0.250 0.125 3 0.200 0.100 4 0.350 0.100 5 0.175 0.100 The initial rate of the first reaction was 0.310 mol/L min. The second reaction was one half that rate, the third reaction was one third times the rate of the first reaction, and the fourth reaction was 0.17 times the rate of the first reaction. The fifth reaction was half the rate of the forth reaction. Determine the value for the constant k.Answer the following questions based on the reaction profile provided in the image: 1. How many elementary reactions are in the reaction mechanism? 2. What is the enthalpy of the overall forward reaction A→D (Endo or Exo)?The reaction rate of the following reaction:aA +bB ==> cC is known to be:k[A] 0 [B]2 Now answer the following question(s): In one trial reaction the initial concentration of A was 7.56e8 M. By what factor would the rate change, if [A] is decreased to 2.52e8 M in a second trial? In one trial reaction the initial concentration of B was 3.77e8 M. By what factor would the rate change, if [ B] is decreased to 1.26e8 M in a second trial?
- Please show all your work please, thank you! Sorry, this question has many parts. The reaction O3(g)+O(g)→2O2(g), occurs via the following mechanism:Step 1: Cl(g)+ O3(g)→ClO(g)+O2(g); Ea=85 kJ/molStep 2: ClO(g)+ O(g)⇌Cl(g)+O2(g); Ea=10 kJ/mol a. Given the proposed mechanism above, identify any catalysts and any intermediates in this reaction. Be sure to distinguish between the two types of species in your answer. b. Using the proposed mechanism, derive a rate law. *Hint: use the activation energies to determine the slower step. Show all of your work. c. This mechanism was verified by kinetic measurements of the rate of depletion of ozone. How is the rate of change of oxygen gas concentration related to the rate of change of ozone concentration? d. Use the standard enthalpies of formation given below to determine the change in enthalpy for the reaction, Δ?°. e. Sketch a reaction diagram for this reaction. You should have energy on the vertical axis and reaction progress on the…The following initial rate data are for the reduction of nitric oxide with hydrogen:2 NO + 2 H2N2 + 2 H2O Experiment [NO]o, M [H2]o, M Initial Rate, M s-1 1 0.160 0.420 1.57×10-2 2 0.320 0.420 6.28×10-2 3 0.160 0.840 3.14×10-2 4 0.320 0.840 0.126 Complete the rate law for this reaction in the box below.Use the form k[A]m[B]n , 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-1The following questions refer to the gas-phase decomposition of ethylene chloride. C2H5Cl → products Experiment shows that the decomposition is first order. The following data show kinetics information for this reaction: Time (s) ln [C2H5Cl] (M) 1.0 –1.625 2.0 –1.735 What is the rate constant for this decomposition? *Side note: The answer to this problem is 0.11/s but I am unsure how to get there.*
- A2 Please write down the reaction mechanismBe sure to answer all parts. Consider the reaction 4PH3(g) → P4(g) + 6H2(g) Suppose that, at a particular moment during the reaction, molecular hydrogen is being formed at rate of 0.239 M/s. (a) At what rate is P4 changing? M/s (b) At what rate is PH3 changing? M/sFPlease answer part b. Nitric oxide gas (NO) reacts with chlorine gas according to the equation NO + ½Cl2 à NOCl. The following initial rates of reaction have been measured for the given reagent concentrations. Expt. # Rate (M/hr) NO (M) Cl2(M) 1 1.19 0.50 0.50 2 4.79 1.00 0.50 3 9.59 1.00 1.0 a) Determine the order of the reaction with respect to the NO and Cl2. b) Calculate the rate constant. Be sure to give the correct units.
- For a reaction, A → products, with the rate law: Rate = k[A]2, (a) a plot of ln[A] vs. time gives a straight line. (b) a plot of Rate vs. concentration gives a straight line. (c) both (a) and (b) are correct. (d) a plot of 1/[A] vs. time gives a straight line. (e) both (b) and (d) are correct.hemistry the order of the reaction is n=12. The initial rate of a reaction A + B → C was measured for several different starting concentrations of A and B, and the results are as follows: Experiment Number [A] (M) [B] (M) Initial Rate (M/s) 1 0.100 0.100 4.0x10-5 2 0.200 0.200 4.0x10-5 3 0.200 0.100 16.0x10-5 Using these data, determine (a) the rate law for the reaction, (b) the rate constant, (c) the rate of the reaction when [A] = 0.050 M and [B] = 0.100 M.