Standard Heat of Reaction Equation:
From: | To: |
The standard heat of reaction (ΔH°) is the change in enthalpy that occurs in a chemical reaction under standard conditions. It indicates whether a reaction is exothermic (releases heat, ΔH° < 0) or endothermic (absorbs heat, ΔH° > 0).
The calculator uses the standard heat of reaction equation:
Where:
Explanation: The equation calculates the difference between the total enthalpy of the products and the total enthalpy of the reactants under standard conditions.
Details: Calculating standard heat of reaction is essential for understanding reaction thermodynamics, predicting reaction spontaneity, and designing chemical processes in industry.
Tips: Enter the sum of standard heats of formation for products and reactants in kJ/mol. The calculator will compute the standard heat of reaction.
Q1: What are standard conditions?
A: Standard conditions are typically 1 atm pressure and 25°C (298 K) for thermodynamic calculations.
Q2: Where can I find ΔHf values?
A: Standard heats of formation are tabulated in thermodynamic reference books and databases like the NIST Chemistry WebBook.
Q3: What does a negative ΔH mean?
A: A negative ΔH indicates an exothermic reaction (releases heat to surroundings), while positive ΔH indicates endothermic reaction (absorbs heat).
Q4: Does this apply to all reactions?
A: This calculation applies to reactions where all reactants and products are in their standard states. For non-standard conditions, additional corrections are needed.
Q5: How does this relate to Gibbs free energy?
A: While ΔH measures heat change, Gibbs free energy (ΔG = ΔH - TΔS) determines reaction spontaneity by also considering entropy change (ΔS).