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Enthalpy change is the heat absorbed or released in a chemical reaction at constant pressure, and it is symbolized by ΔH. It is a key concept in thermodynamics, helping indicate whether a reaction is exothermic (releases heat) or endothermic (absorbs heat). Understanding enthalpy change is crucial for predicting how different reactions behave, making it an essential topic for students studying chemistry.
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Sign up for freeHow is the change in enthalpy (\(\triangle H\)) calculated?
What does enthalpy change (\(\triangle H\)) represent in engineering?
What does the symbol \(H\) represent in thermodynamics?
What does a negative \(\triangle H\) indicate?
What is the standard enthalpy change of formation for pure elements in their most stable form?
Why is understanding enthalpy change important in engineering?
How do you calculate reaction enthalpies using enthalpy of formation?
Which of the following systems benefit from understanding enthalpy change?
What indicates an exothermic reaction based on enthalpy change?
How do enthalpy changes apply to engineering?
What is the basic formula for calculating enthalpy change?
How is the change in enthalpy (\(\triangle H\)) calculated?
What does enthalpy change (\(\triangle H\)) represent in engineering?
What does the symbol \(H\) represent in thermodynamics?
What does a negative \(\triangle H\) indicate?
What is the standard enthalpy change of formation for pure elements in their most stable form?
Why is understanding enthalpy change important in engineering?
How do you calculate reaction enthalpies using enthalpy of formation?
Which of the following systems benefit from understanding enthalpy change?
What indicates an exothermic reaction based on enthalpy change?
How do enthalpy changes apply to engineering?
What is the basic formula for calculating enthalpy change?
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Understanding enthalpy change is crucial in the field of engineering. It describes the thermodynamic potential to do non-mechanical work and the amount of energy in a system capable of doing this work during a constant-pressure process.
Enthalpy change, often denoted as \(\triangle H\), refers to the heat absorbed or released in a chemical reaction at constant pressure. It is measured in joules or calories.
Enthalpy change is used to calculate the heat transfer during phase changes, chemical reactions, and other processes where energy is transferred.Some common scenarios where you might encounter enthalpy change include:
Think of enthalpy as a measure of thermal energy in a system at constant pressure.
The change in enthalpy \(\triangle H\) can be calculated using the formula: \[\triangle H = H_{final} - H_{initial}, \] where \(H_{final}\) is the enthalpy of the products and \(H_{initial}\) is the enthalpy of the reactants. For reactions carried out at constant pressure, the enthalpy change is equivalent to the heat absorbed or released.
For a chemical reaction \(C + O_2 \rightarrow CO_2\), if the enthalpy of the reactants (carbon and oxygen) is \(394 \, kJ \, mol^{-1}\) and the products (carbon dioxide) is \(0 \, kJ \, mol^{-1}\), the enthalpy change would be: \[\triangle H = 0 - 394 = -394 \, kJ \, mol^{-1}.\] This indicates an exothermic reaction.
In engineering, understanding enthalpy change is essential for designing efficient energy systems. For example, in heat engines, turbines, and refrigerators, enthalpy changes explain how much energy is lost as waste heat versus amount converted into mechanical work. The second law of thermodynamics is often referenced with enthalpy change, as it describes inefficiencies and increased entropy in energy transformations. Detailed calculations involving enthalpy changes allow you to optimize these systems for maximum efficiency.
To understand enthalpy change in engineering, you must familiarize yourself with the formula and the concept behind it. It's a fundamental aspect of thermodynamics, often used in designing and evaluating energy systems.
The enthalpy change \(\triangle H\) is defined as the difference in enthalpy between products and reactants, calculated as \[\triangle H = H_{products} - H_{reactants}\]. Enthalpy itself is represented by the symbol \(H\) and is measured in joules or calories.
In reactions at constant pressure, the enthalpy change equates to the heat exchanged. The sign of \(\triangle H\) indicates whether the reaction is exothermic (negative \(\triangle H\)) or endothermic (positive \(\triangle H\)).
Consider the formation of water from hydrogen and oxygen: \(2H_2 + O_2 \rightarrow 2H_2O\). If the enthalpies of the reactants and products are \(0 \, kJ \, mol^{-1}\) and \(-572 \, kJ \, mol^{-1}\) respectively, calculate \(\triangle H\):\[\triangle H = -572 \, kJ \, mol^{-1} - 0 \, kJ \, mol^{-1} = -572 \, kJ \, mol^{-1}\] This shows the reaction is exothermic.
Understanding enthalpy changes is crucial for various engineering applications, such as:
In steam engines, for example, enthalpy change defines how much of the steam's energy is convertible into work. Engineers need to account for enthalpy changes to minimize energy loss and improve system efficiency. Moreover, advancements in renewable energy technology often rely on enthalpy calculations to maximize resource use. Enthalpy changes influence the energy balance in systems like solar panels and wind turbines, playing a significant role in their development.
Remember that the standard state conditions for measuring enthalpy are 298 K, 1 atm pressure, and, often, a concentration of 1 M for all solutions.
The Standard Enthalpy Change of Formation is an essential concept in engineering thermodynamics. It represents the heat change that occurs when one mole of a compound is formed from its elements in their standard states at 298 K and 1 atm pressure.
Standard Enthalpy Change of Formation (\(\triangle H_f^\circ\)) is defined as the enthalpy change when one mole of a compound is formed from its elements under standard conditions. This is typically measured in \(\text{kJ} \, \text{mol}^{-1}\).
Consideration of standard enthalpy change of formation is vital in various chemical processes for evaluating reaction energetics. For example, it helps predict reaction spontaneity via the calculation of Gibbs free energy.
For formation of water (\(H_2O\)) from its elements (\(H_2\) and \(O_2\)), the standard enthalpy change of formation is given by:\[- \triangle H_f^\circ \, = -285.8 \, \text{kJ mol}^{-1}\]This indicates releasing heat and is typically exothermic.
Standard enthalpy of formation for pure elements in their most stable forms is zero (\(\triangle H_f^\circ = 0\)).
Calculating reaction enthalpies using the enthalpy of formation involves the following formula:\[\triangle H_{reaction} = \sum \triangle H_f^\circ (products) - \sum \triangle H_f^\circ (reactants)\]This allows determination of the overall heat exchange in reactions where enthalpies of individual components are known.An example involves calculating the enthalpy change of the reaction:
The standard enthalpy change of formation not only aids in evaluating current processes but also helps in research and development of alternative fuel sources. Biofuels, for example, strive to match or surpass traditional fossil fuels, not only in energy output but also in sustainable heat production and minimal environmental impact. Studying the enthalpy of formation in renewable energy sources, like hydrogen fuel cells, is pivotal to pushing forward with innovations that can harness clean energy solutions. By optimizing these values, the efficiency of energy production and consumption can see significant advancements, consistently aligning with global sustainability goals.
Calculating the enthalpy change is a fundamental skill in thermodynamics, allowing you to analyze the energy transformations that occur in chemical reactions.
To determine the enthalpy change of a reaction, you must consider the enthalpy of products and reactants. The basic formula for calculating enthalpy change is:\[\triangle H = H_{products} - H_{reactants}\]This calculation is performed at constant pressure, where heat exchange occurs without changes in volume. A key consideration is whether the reaction is exothermic or endothermic.
For an exothermic reaction such as the combustion of methane:\(CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O\)Suppose the enthalpy values are:
Enthalpy change, denoted by \(\triangle H\), represents the heat absorbed or released during a chemical reaction at constant pressure. It is expressed in \(\text{kJ mol}^{-1}\). A negative \(\triangle H\) suggests an exothermic reaction, while a positive value indicates an endothermic process.
Remember: in any calculation, maintaining consistent units, such as joules or calories, is essential when comparing enthalpy changes across different reactions.
In advanced engineering applications, understanding enthalpy change is critical for designing processes that optimize heat utilization. For example, in power plants, engineers leverage enthalpy columns to analyze steam cycles, balancing enthalpy changes throughout the system for maximum efficiency. By calculating specific enthalpy along various states (pressures and temperatures), engineers can refine system designs, minimize waste, and enhance output. Beyond classical engines, emerging technologies such as concentrated solar power systems utilize precise enthalpy calculations to store and convert solar energy highly efficiently.
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