Physical chemistry solving problem
1. Consider the following theoretical reaction.
Assuming the rate of the reaction (r) and the concentration of the reactant ([A]) can be measured over time
(that is the r vs. [A] data is available), what plot would you propose to make to determine the order (x),
and the rate constant (k)?
SHOW YOUR ANSWER STEP BY STEP AND SPECIFIC
2. Using the provided spreadsheet for consecutive reaction, generate graphs for the following
situations and interpret them (and paste them here as images):
OPEN EXCEL FILE IN PROBLEM 2, AND PLAY WITH K1, K2, T VALE TO CREATE THE GRAPH IN EACH CASE BELOW, COPY THE
GRAPF IN THIS WORD FILE
• First step is rate determining
• Second step is rate determining
• The two rate constants are comparable
Identify and justify the situation where the steady-state approximation can be used.
3. Bromophenol blue (Bp) reacts with sodium hydroxide according to the following reaction.
The reactant (Bp) is blue, the product is colorless, therefore the reaction can be followed by
spectrophotometry. Two runs were performed with the initial hydroxide concentrations [OH-]1,0 = 1.00M and
[OH-]2,0 = 2.00M. For both runs the concentration of Bromophenol blue was [Bp]0 = 1.2×10-5M. The A vs. time
data for both runs are given in the Excel file.
OPEN EXCEL FILE IN PROBLEM 3, USE THE DATA TO GRAPH IN EXCEL FILE , AND CALCULATE THE Q A,B,C,D STEP BY STEP
IN WORD FILE
a.) Determine the order of [Bp] in the reaction.
b.) Determine the order of [OH-] in the reaction.
c.) Determine the rate constant, k, of the reaction.
d.) Interpret the effect of [OH]>>[Bp] in terms of the mechanism of the reaction.
4. The isomerization of ammonium cyanate to urea was followed in aqueous solution initially containing
22.9g of ammonium cyanate (FW = 60 g/mol) in 1.00L solution.
The amount of urea formed as a function of time is provided in the Excel file.
OPEN THE EXCEL FILE PROBLEM 4, USE THAT DATA, AND CALCULATION IN EXCEL, WITH YOUR CALCULATION FILE. ANSWER 1
AND 5 STEP BY STEP AND SPECIFIC
a.) Order of reaction for ammonium cyanate
b.) Rate constant (use min for time unit)
5. The decomposition of ethylamine was followed at different temperatures.
The values of the total pressure as a function of time at three different temperatures are provided in the
Excel file. The worksheet is setup for your convenience, but you do not have to use it. Each cell with a red
triangle in the top right corner has information for you, just hover over the cell with your mouse to see
(Hint: First, calculate the partial pressure of the reactant at each point using the ICE box. Then calculate
the rate constant for each temperature using the appropriate integrated rate equation. Finally, use the
Arrhenius equation for the activation energy and pre-exponential coefficient).
a.) Order of the reaction
b.) Rate constants at different temperatures
c.) Energy of activation
d.) Pre-exponential coefficient
6. The decomposition of gamma-hydroxy-butirate (GHB) was studied in the presence of 5.0 nM chymotripsin
and with and without 6.0 mM ethanol.
a.) What is the value of the Michaelis constant (KM), the turnover frequency (kcat), and the catalytic
efficiency (?) in the presence and in the absence of ethanol, and the equilibrium constant for the
dissociation of EIS (KI)?
b.) b) Does the alcohol act as an inhibitor, and if so, through what mechanism?
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