Data in the table below were collected at 25°C for the following reaction: 2 (aq) + S20, 2- (aq) - 12 (aq) + 2 SOs*(aq) Initial concentration (mol-dm-) Initial rate (mol-dm ³s*) Exp (S:0, 21 1. 0.080 0.040 12.5 x 104 2 0.040 0.040 6.25 x 10 3 0.080 0.020 6.25 x 10 4 0.032 0.040 5.00 x 106 0.060 0.030 7.00 x 10 a) Determine the rate law for the reaction. b) Calculate the rate constant, giving the correct units for k.

Question 9 The following data were obtained for a reaction. What is the activation energy? R-8.314 J/Kmol; T(K) - T("C) + 273 Report your answer in kJ to one decimal place. Trial Rate constant Temperature ("c) 1. 4.97 x 10- 36 2 6.59 x 10- 113 Answer:

Dinitrogen pentoxide rapidly decomposes in the atmosphere with the rate law noted. 2 N₂O5 (g) → 4 NO2 (g) + O₂(g) rate= (5.85 × 10-³s-¹) [N₂05] S How long does it take for sample to decompose from an initial concentration of 0.750M to0.211M ? Answer formatting tip: enter the reaction time using three significant figures; omit the units of s.

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Cindy decomposed a metal hydroxide via the reation: Mt(OH) 3 → MtO + H20, and then collected concentration and time data. After analyzing on her TI84 the following data were obtained. [Mt(OH)3] vs. time a = 2.10 x 104 In[Mt(OH)3] vs. time a = -5.80 x 10-5 b = -0.770 r = 0.999 [Mt(OH)3] vs. time a = -1.72 x 10-5 b = 0.450 r = 0.917 2.00 %3D r² 0.981 What is the order with respect to Mt(OH)3? What is the value of the rate constant for this reaction?

O https://app.101edu.co A * Question 7 of 20 Determine the rate law for the reaction A+ B - C + D given the following experiment data. Initial Trial [A]o [B]o Rate A) Rate = k[A] %3D (M/min) B) Rate = k[A]? 1 0.25 0.40 7.25 C) Rate = k[A][B] %3D 2 0.75 0.40 21.5 D) Rate = k[A]°[B] %3D 3 0.50 0.80 14.5 E) Rate = k[A][B] 4 0.75 0.80 21.5 Delete F12 wwwn D F11 FI0 FO FB FS FO Backspace Num Lock F2 %3D 1 8. 6. 4 12 3 Wome E R Enter J K F S. Shift Poyblip Ctr Alt Home All

For the question above, calculate the value of k (include units). Show your work.

Question: Calculate the thermodynamic favorability of aerobic Mn (II) oxidation and aerobic Fe(II) oxidation at pH 2 and 7. Is it likely that an organism could get enough "energy" to grow from each of these four processes?

Which equation best describes the average rate for the reaction shown? A(aq) + B(aq) → C(aq) + D(aq)   Multiple Choice   rate = [C][D] [A][B]   rate = +Δ[B]/Δt   rate = –Δ[C]/Δt   rate = –Δ[A]/Δt   rate = [A][B] [C][D]