CHEM 104 KINETICS EXPERIMENT 1 SUMMER 3
2026 COMPREHENSIVE CHEMISTRY LAB
REVIEW QUESTIONS AND SOLUTIONS
VERIFIED
◉ From the experiment section, you will determine three things:
1. the kinetic order with respect to H2O2 (at room temp.)
2. the kinetic order with respect to KI (at room temp.)
3. the energy of activation, conducted at three different
temperatures (in addition to the room temp. trial).
How many trials are needed to determine parts 1 and 2? And, by
how many Kelvin (K) should the temperatures vary for part 3?
Answer: 9 trials; ~10 K
◉ From the "Planning your Experiments" section: the procedure for
trial #1 is outlined in the manual.
You'll need:
2 mL of 0.88 M H2O2
1 mL of 0.50 M KI
To determine the order for each reactant (the remaining trials, #2-
9), you need to change only ONE concentration at a time.
If KI is kept constant, you will make up a new dilution of H2O2 in a
small graduated cylinder and will transfer only _______ mL of the new
, solution to the reaction flask so that the total volume in the reaction
flask is constant at _______ mL. Answer: 2 mL; 3 mL
◉ Start the data analysis as early as possible.
For each trial, you'll be provided with the slope of the pressure vs.
time graph.
This slope must be converted (using the ideal gas law) to give you
the rate of the reaction.
Once you have the rates, how are the reaction orders "a" and "b"
determined? Answer: Graphically, by plotting H2O2 and KI
separately.
◉ objective Answer: To monitor the rate of a chemical reaction, to
determine the kinetic order of a reaction from dependence of the
rate on reactant concentrations, to understand how the molecular
components of the rate limiting step of the reaction are determined
by the kinetic order of the reaction and to determine the energy of
activation (Ea) of the reaction from the temperature dependence of
the reaction rate.
◉ key equation Answer: rate = k[H2O2]a[KI]b
This is the rate law, where k is the rate constant (which changes with
temperature)
2026 COMPREHENSIVE CHEMISTRY LAB
REVIEW QUESTIONS AND SOLUTIONS
VERIFIED
◉ From the experiment section, you will determine three things:
1. the kinetic order with respect to H2O2 (at room temp.)
2. the kinetic order with respect to KI (at room temp.)
3. the energy of activation, conducted at three different
temperatures (in addition to the room temp. trial).
How many trials are needed to determine parts 1 and 2? And, by
how many Kelvin (K) should the temperatures vary for part 3?
Answer: 9 trials; ~10 K
◉ From the "Planning your Experiments" section: the procedure for
trial #1 is outlined in the manual.
You'll need:
2 mL of 0.88 M H2O2
1 mL of 0.50 M KI
To determine the order for each reactant (the remaining trials, #2-
9), you need to change only ONE concentration at a time.
If KI is kept constant, you will make up a new dilution of H2O2 in a
small graduated cylinder and will transfer only _______ mL of the new
, solution to the reaction flask so that the total volume in the reaction
flask is constant at _______ mL. Answer: 2 mL; 3 mL
◉ Start the data analysis as early as possible.
For each trial, you'll be provided with the slope of the pressure vs.
time graph.
This slope must be converted (using the ideal gas law) to give you
the rate of the reaction.
Once you have the rates, how are the reaction orders "a" and "b"
determined? Answer: Graphically, by plotting H2O2 and KI
separately.
◉ objective Answer: To monitor the rate of a chemical reaction, to
determine the kinetic order of a reaction from dependence of the
rate on reactant concentrations, to understand how the molecular
components of the rate limiting step of the reaction are determined
by the kinetic order of the reaction and to determine the energy of
activation (Ea) of the reaction from the temperature dependence of
the reaction rate.
◉ key equation Answer: rate = k[H2O2]a[KI]b
This is the rate law, where k is the rate constant (which changes with
temperature)
