Enthalpy Change of Neutralisation Calculator
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Enthalpy change of neutralisation is a crucial concept in thermochemistry that measures the energy change when an acid and a base react to form water. It helps in understanding the heat exchange in neutralisation reactions.
Historical Background
The study of enthalpy change of neutralisation dates back to the development of thermodynamics in the 19th century. Scientists like Hess and Lavoisier contributed significantly to understanding how energy is conserved in chemical reactions. The concept is widely applied in calorimetry to determine heat changes during acid-base reactions.
Calculation Formula
The enthalpy change of neutralisation is calculated using the formula:
\[ \Delta H_{\text{neut}} = \frac{Q}{n} \]
where:
- \(\Delta H_{\text{neut}}\) is the enthalpy change of neutralisation (kJ/mol),
- \(Q\) is the heat energy released (kJ),
- \(n\) is the number of moles of water formed (mol).
Example Calculation
If a neutralisation reaction releases 50 kJ of heat energy and produces 2 moles of water, the enthalpy change is:
\[ \Delta H_{\text{neut}} = \frac{50}{2} = 25 \text{ kJ/mol} \]
Importance and Usage Scenarios
- Laboratory experiments: Used in calorimetry to measure reaction heat changes.
- Industrial applications: Helps in designing energy-efficient acid-base neutralisation processes.
- Educational purposes: A fundamental concept in chemistry and thermodynamics courses.
Common FAQs
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Why is the enthalpy change of neutralisation always negative?
- Because neutralisation is an exothermic reaction, meaning heat is released to the surroundings.
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Does the type of acid or base affect the enthalpy change?
- Strong acid-strong base reactions generally have similar enthalpy changes, while weak acids or bases may show variations due to partial ionisation.
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How is enthalpy change measured experimentally?
- By using a calorimeter to measure temperature changes in a known volume of solution.
This calculator simplifies the process of determining the enthalpy change of neutralisation, making it a valuable tool for students, researchers, and industry professionals.