Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
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

Using the Arrhenius Equation, what is the rate constant (k) for the reaction of NO with F2 at a temperature of 298 K, given that the activation energy (Ea) is 6.30 kJ/mol and the frequency factor (A) is 6.00 × 10^8 M⁻¹·s⁻¹?

k = 5.67 × 10^9 M⁻¹·s⁻¹

k = 4.56 × 10^8 M⁻¹·s⁻¹

k = 1.23 × 10^7 M⁻¹·s⁻¹

k = 2.45 × 10^7 M⁻¹·s⁻¹

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Verified step by step guidance

Start by recalling the Arrhenius Equation, which is used to calculate the rate constant (k) of a reaction: \( k = A \cdot e^{-\frac{E_a}{RT}} \), where \( A \) is the frequency factor, \( E_a \) is the activation energy, \( R \) is the universal gas constant, and \( T \) is the temperature in Kelvin.

Convert the activation energy \( E_a \) from kJ/mol to J/mol to match the units of the gas constant \( R \). Since 1 kJ = 1000 J, multiply 6.30 kJ/mol by 1000 to get 6300 J/mol.

Use the universal gas constant \( R = 8.314 \) J/(mol·K) and the given temperature \( T = 298 \) K in the Arrhenius equation.

Substitute the values into the Arrhenius equation: \( k = 6.00 \times 10^8 \cdot e^{-\frac{6300}{8.314 \times 298}} \).

Calculate the exponent \( -\frac{6300}{8.314 \times 298} \), then find the value of \( e \) raised to this power, and finally multiply by the frequency factor \( A = 6.00 \times 10^8 \) to find the rate constant \( k \).