“Comprehensive Advanced University
Chemistry Randomized Question Pool
Featuring Activation Energy, Reaction
Kinetics, Thermodynamics, and
Molecular Theory with Detailed Answers
and Explanations for Mastery.”
VATI Activation Energy Lab Report
Title:
Determining the Activation Energy of a Chemical Reaction
Objective:
To determine the activation energy (Ea) of a reaction by
measuring how the rate constant (k) changes with temperature
and applying the Arrhenius equation
Background Theory:
The activation energy (Ea) is the minimum energy required for
reactants to form products in a chemical reaction. The
relationship between the rate constant and temperature is given
by the Arrhenius Equation:
,[
k = A e^{-E_a / (RT)}
]
Where:
• ( k ) = rate constant
• ( A ) = frequency factor (collision factor)
• ( E_a ) = activation energy (J/mol)
• ( R ) = universal gas constant (8.314 J/mol·K)
• ( T ) = temperature (K)
Taking the natural logarithm of both sides gives a linear form:
[
\ln(k) = -\frac{E_a}{R}\left(\frac{1}{T}\right) + \ln(A)
]
This linear relationship allows for determination of ( E_a ) from
the slope of a plot of ( \ln(k) ) vs. ( 1/T ).
Materials and Equipment:
• VATI simulation environment (Activation Energy Lab
module)
• Stopwatch (virtual)
• Temperature control interface
• Graphing tool or software (Excel, Google Sheets, or built-
in VATI analysis tool)
,Procedure:
1. Open the VATI Activation Energy simulation.
2. Select the reaction system (commonly, a hydrogen
peroxide decomposition or iodine clock reaction).
3. Set the initial temperature and record the time taken for
the reaction to complete or the rate constant (k)
displayed.
4. Repeat the simulation at five different temperatures (e.g.,
20°C, 30°C, 40°C, 50°C, 60°C).
5. Convert all temperatures to Kelvin (T = °C + 273).
6. Record the corresponding rate constants (k) for each
temperature.
7. Calculate ln(k) and 1/T for each trial.
8. Plot ln(k) (y-axis) versus 1/T (x-axis).
9. Determine the slope (m) of the best-fit line.
10. Calculate activation energy (Ea) using the
relationship:
[
E_a = -m \times R
]
Data Table:
Temperature Temperature Rate 1/T
ln(k)
(°C) (K) Constant (k) (K⁻¹)
-
20 293 0.012 0.00341
4.42
-
30 303 0.018 0.00330
4.02
, Temperature Temperature Rate 1/T
ln(k)
(°C) (K) Constant (k) (K⁻¹)
-
40 313 0.027 0.00319
3.61
-
50 323 0.040 0.00310
3.22
-
60 333 0.059 0.00300
2.83
Graph:
Plot of ln(k) versus 1/T yields a straight line with a negative
slope.
[
\text{slope} = -E_a / R
]
(You can include your VATI graph screenshot or attach a
plotted graph from Excel.)
Calculations:
From linear regression, suppose the slope = -5420 K.
[
E_a = -(\text{slope}) \times R = (5420)(8.314) = 45,200 \text{
J/mol} = 45.2 \text{ kJ/mol}
]
Chemistry Randomized Question Pool
Featuring Activation Energy, Reaction
Kinetics, Thermodynamics, and
Molecular Theory with Detailed Answers
and Explanations for Mastery.”
VATI Activation Energy Lab Report
Title:
Determining the Activation Energy of a Chemical Reaction
Objective:
To determine the activation energy (Ea) of a reaction by
measuring how the rate constant (k) changes with temperature
and applying the Arrhenius equation
Background Theory:
The activation energy (Ea) is the minimum energy required for
reactants to form products in a chemical reaction. The
relationship between the rate constant and temperature is given
by the Arrhenius Equation:
,[
k = A e^{-E_a / (RT)}
]
Where:
• ( k ) = rate constant
• ( A ) = frequency factor (collision factor)
• ( E_a ) = activation energy (J/mol)
• ( R ) = universal gas constant (8.314 J/mol·K)
• ( T ) = temperature (K)
Taking the natural logarithm of both sides gives a linear form:
[
\ln(k) = -\frac{E_a}{R}\left(\frac{1}{T}\right) + \ln(A)
]
This linear relationship allows for determination of ( E_a ) from
the slope of a plot of ( \ln(k) ) vs. ( 1/T ).
Materials and Equipment:
• VATI simulation environment (Activation Energy Lab
module)
• Stopwatch (virtual)
• Temperature control interface
• Graphing tool or software (Excel, Google Sheets, or built-
in VATI analysis tool)
,Procedure:
1. Open the VATI Activation Energy simulation.
2. Select the reaction system (commonly, a hydrogen
peroxide decomposition or iodine clock reaction).
3. Set the initial temperature and record the time taken for
the reaction to complete or the rate constant (k)
displayed.
4. Repeat the simulation at five different temperatures (e.g.,
20°C, 30°C, 40°C, 50°C, 60°C).
5. Convert all temperatures to Kelvin (T = °C + 273).
6. Record the corresponding rate constants (k) for each
temperature.
7. Calculate ln(k) and 1/T for each trial.
8. Plot ln(k) (y-axis) versus 1/T (x-axis).
9. Determine the slope (m) of the best-fit line.
10. Calculate activation energy (Ea) using the
relationship:
[
E_a = -m \times R
]
Data Table:
Temperature Temperature Rate 1/T
ln(k)
(°C) (K) Constant (k) (K⁻¹)
-
20 293 0.012 0.00341
4.42
-
30 303 0.018 0.00330
4.02
, Temperature Temperature Rate 1/T
ln(k)
(°C) (K) Constant (k) (K⁻¹)
-
40 313 0.027 0.00319
3.61
-
50 323 0.040 0.00310
3.22
-
60 333 0.059 0.00300
2.83
Graph:
Plot of ln(k) versus 1/T yields a straight line with a negative
slope.
[
\text{slope} = -E_a / R
]
(You can include your VATI graph screenshot or attach a
plotted graph from Excel.)
Calculations:
From linear regression, suppose the slope = -5420 K.
[
E_a = -(\text{slope}) \times R = (5420)(8.314) = 45,200 \text{
J/mol} = 45.2 \text{ kJ/mol}
]
