1. What is the Arrhenius Equation?

The Arrhenius equation describes the temperature dependence of reaction rates. It shows how the rate constant changes with temperature, helping predict reaction rates at different temperatures.

2. How Does the Calculator Work?

The calculator uses the Arrhenius equation:

Where:

• \( k_1 \) — Rate constant at temperature T₁ (1/s)
• \( k_2 \) — Rate constant at temperature T₂ (1/s)
• \( E_a \) — Activation energy (J/mol)
• \( R \) — Universal gas constant (8.314 J/mol·K)
• \( T_1 \) — Initial temperature (K)
• \( T_2 \) — New temperature (K)

Explanation: The equation shows that reaction rates increase exponentially with temperature, with the activation energy determining how sensitive the rate is to temperature changes.

3. Importance of the Arrhenius Equation

Details: The Arrhenius equation is fundamental in chemical kinetics, used to predict shelf life of products, design chemical processes, and understand biological reactions.

4. Using the Calculator

Tips: Enter all values in the specified units. Temperatures must be in Kelvin. The calculator will compute the rate constant at the new temperature (k₂).

5. Frequently Asked Questions (FAQ)

Q1: How do I convert Celsius to Kelvin?
A: Add 273.15 to the Celsius temperature to get Kelvin.

Q2: What is a typical activation energy range?
A: Most chemical reactions have Eₐ between 50-250 kJ/mol (50,000-250,000 J/mol).

Q3: Why does the rate constant increase with temperature?
A: Higher temperatures provide more energy to overcome the activation energy barrier, leading to more successful collisions.

Q4: Can this be used for biological systems?
A: Yes, but with caution as enzyme-catalyzed reactions may deviate from Arrhenius behavior at extreme temperatures.

Q5: What's the relationship between rate constant and reaction rate?
A: Reaction rate = rate constant × concentration terms, so the rate constant determines how fast the reaction proceeds at given concentrations.