Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 36m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

15. Chemical Kinetics

Arrhenius Equation

General Chemistry

15. Chemical Kinetics

Arrhenius Equation

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Multiple Choice

By what factor is the rate of a reaction changed if an enzyme lowers the activation energy (Ea) by 7.0 kJ/mol at 37°C, according to the Arrhenius Equation?

Approximately 2 times

Approximately 5 times

Approximately 10 times

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Verified step by step guidance

Understand that the Arrhenius Equation is given by: \( k = A e^{-\frac{E_a}{RT}} \), where \( k \) is the rate constant, \( A \) is the pre-exponential factor, \( E_a \) is the activation energy, \( R \) is the gas constant (8.314 J/mol·K), and \( T \) is the temperature in Kelvin.

Convert the temperature from Celsius to Kelvin: \( T = 37 + 273.15 = 310.15 \text{ K} \).

Calculate the change in the exponent of the Arrhenius equation due to the change in activation energy: \( \Delta E_a = 7.0 \text{ kJ/mol} = 7000 \text{ J/mol} \).

Determine the factor by which the rate changes using the ratio of the rate constants: \( \frac{k_2}{k_1} = e^{\frac{\Delta E_a}{RT}} \). Substitute \( \Delta E_a = 7000 \text{ J/mol} \), \( R = 8.314 \text{ J/mol·K} \), and \( T = 310.15 \text{ K} \) into the equation.

Calculate the exponential term to find the factor by which the rate changes: \( e^{\frac{7000}{8.314 \times 310.15}} \). This will give you the approximate factor by which the rate of the reaction is increased.