EES 6208 University of Washington Water Chemistry & Elementary Reactions Lab Report
I’m trying to study for my Chemistry course and I need some help to understand this question.
Problem-1: A reversible reaction that is elementary in both directions has the following stoichiometry:
Hydroxide ion has been found to catalyze (i.e., to increase the rate of) the forward reaction. How would the following parameters change when the pH is increased? Briefly explain your reasoning.
- The activation energy for the forward reaction (5 points).
- The rate constant for the reverse reaction (5 points).
Problem-2: A network of elementary reactions is shown below, along with rate constants for the forward (f) and reverse (r) of each reaction. Note that species A is consumed in reactions 1 and 2, and is then generated in reaction 3. Similarly, species D is generated in reaction 2 and then consumed in reaction 3. The rate constants apply when the species’ activities (not their concentrations) are used in the reaction rate expressions. The units of ‘mol’ refer to moles of stoichiometric reaction.
- Write the overall reaction corresponding to the sum of these elementary reactions and determine the equilibrium constant that applies to that reaction (15 points).