Derivation The Arrhenius equation can be written as: k = Ae Consider a reaction with some activation energy that we will call Ea1-Suppose a catalyst is added to the reaction that binds to the transition state and lowers the activation energy to a new E, that we can call E 2. We can define the difference in catalyzed and uncatalyzed activation energies as AEG-Ea2-E1- The rate enhancement due to the presence of a catalyst can be defined as where k₁ is the rate constant of the reaction without the catalyst, and k2 is the rate constant of t process with the catalyst, both at some constant temperature T. Derive an expression for the rate enhancement in terms of T and AE, and select an equivalent equation from the list below. k²= In (46) O O k₂ AE =eR = In (e 12 = 46 ) = In (AF)

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of : Suppose a flask is charged under these conditions with of hydrogen iodide. How much is left later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.

The starting concentration (time zero) of crystal violet is 1 x 10-4 M. Using the proper integrated rate law and the calculated value for k, calculate the concentration of crystal violet after 240 seconds. Look at the equation of the trend line for your lost linear graph and the beer-lambert law.   Equation from graph from NaOH 0.0660M is y= -0.0105x-0.6277

A student follows the Determining the Rate Law for the Crystal Violet-Hydroxide lon Reaction procedure. The stock concentration of sodium hydroxide used in trial 1 is 0.020 M. The stock concentration of sodium hydroxide used in trial 2 is 0.010 M. After graphing the data, the slope of the straight-plot line for trial 1 is -0.0722 and for trial 2 is -0.0712. Calculate the reaction order with respect to hydroxide ion concentration. Give your answer as an integer.