Equilibrium Conversion of Reaction at Initial Temperature Calculator

Formula Used:

\[ K_1 = \frac{K_2}{\exp\left(-\left(\frac{\Delta H_r}{[R]}\right)\left(\frac{1}{T_2} - \frac{1}{T_1}\right)\right)} \]

Thermodynamic Constant at Final Temperature (K₂):

Heat of Reaction per Mole (ΔHᵣ):

J/mol

Final Temperature (T₂):

Initial Temperature (T₁):

Thermodynamic Constant at Initial Temperature (K₁):

Unit Converter ▲

Unit Converter ▼

From:	To:

1. What is Equilibrium Conversion at Initial Temperature?

Definition: This calculator determines the equilibrium constant at initial temperature based on known values at a different temperature and the heat of reaction.

Purpose: It helps chemical engineers and researchers predict how equilibrium constants change with temperature for chemical reactions.

2. How Does the Calculator Work?

The calculator uses the van't Hoff equation:

\[ K_1 = \frac{K_2}{\exp\left(-\left(\frac{\Delta H_r}{[R]}\right)\left(\frac{1}{T_2} - \frac{1}{T_1}\right)\right)} \]

Where:

\( K_1 \) — Equilibrium constant at initial temperature T₁
\( K_2 \) — Equilibrium constant at final temperature T₂
\( \Delta H_r \) — Heat of reaction per mole (J/mol)
\( [R] \) — Universal gas constant (8.314 J/mol·K)
\( T_1 \) — Initial temperature (K)
\( T_2 \) — Final temperature (K)

Explanation: The equation relates the change in equilibrium constant with temperature to the enthalpy change of the reaction.

3. Importance of Equilibrium Conversion Calculation

Details: Understanding how equilibrium constants vary with temperature is crucial for reactor design, process optimization, and predicting reaction yields.

4. Using the Calculator

Tips: Enter the known equilibrium constant (K₂), heat of reaction (ΔHᵣ), and both temperatures in Kelvin. All values must be > 0.

5. Frequently Asked Questions (FAQ)

Q1: What is the significance of the heat of reaction?
A: The heat of reaction (ΔHᵣ) determines how sensitive the equilibrium constant is to temperature changes.

Q2: Why must temperatures be in Kelvin?
A: The equation requires absolute temperature for thermodynamic consistency.

Q3: What does a negative heat of reaction indicate?
A: A negative ΔHᵣ means the reaction is exothermic (releases heat), while positive means endothermic (absorbs heat).

Q4: How accurate is this calculation?
A: It assumes ΔHᵣ is constant over the temperature range. For large ranges, consider temperature-dependent ΔHᵣ.

Q5: Can I use this for any equilibrium reaction?
A: Yes, as long as you have the required parameters, it works for any chemical equilibrium.