3. For the reaction we studied: 21- + S₂08²- - I2 + 2 SO4²- A. Use this value and your experimental activation energy value to draw an energy profile for the reaction with the energies appropriately scaled on the vertical axis. Ea=-58.86 15/mol B. Label AHrxn and Ea on the graph. Energy Reaction Progress → AHrxn = -322 kJ/mol rxn →-322,000 C. Calculate the Ea for the reverse reaction mol

Determine the activation energy of the reaction.

What is the value of the activation energy for this reaction?  _______kJ Is this reaction exothermic or endothermic? _________ What is the value of E for this reaction?  _________kJ

At 40^0c, H202 (aq) will decompose according to the foll. reaction: 2 H202 (aq) ----2H20(l) +02 (g) The foll. data were collected for the concentration of h202 at various times. Time.                    [H202] (mol/L) 0.                           1.600 3.10*10^4              0.592 6.20*10^4.            0.219 (a) Calculate the average rate of decomposition in H202 between0 and 3.10 * 10^4 s. use this rate to calculate the average rate of production 02 (g) over the same time period. (b) What are these rates for the time period 3.10*10^4 s. to 6.20 *10^4 s.? Rate of H202 decomposition Rate of O2 Production

3. Reaction A  products was monitored as a function of time. If a plot of 1/[A] vs. time yield a straight line with slope 0.0050 M-1 s-1. If initial concentration [A]0 = 0.250 M, calculate the concentration of A after 20 seconds

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=64.0 kJ/mol. If the rate constant of this -1 reaction is 0.0021 M - 1 S. at 40.0 °C, what will the rate constant be at -32.0 °C? Round your answer to 2 significant digits. 1 |M - 1 k = •S Ox10

A reaction occurs in two steps with Ea1 = 40 kJ mol-1 and Ea2 = 25 kJ mol-1. The first step is reversible with Ea-1 = 10 kJ mol-1. If the enthalpy change for the overall reaction is -27 kJ mol-1, then what is the activation energy (kJ mol-1) for the reverse of step 2? 065 O 55 082 30 47

Use the References to access important values if needed for this question. The following initial rate data are for the reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution: OCT+1 → or + Cr Experiment [OCI , M Io. M Initial Rate, M 8-¹ 0.00243 0.00184 3.30 × 10-4 0.00243 0.00486 0.00486 1 2 3 4 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for 0.00367 6.58 × 10-4 0.00184 6.60 × 10-4 0.00367 1.32 × 10-³ m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k = M