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Chapter 10: Problem 12

Name two processes for which you could determine an enthalpy change.

Short Answer

Expert verified
Among many processes, enthalpy change can be determined for Combustion and Phase Transitions.

Step by step solution

01

Identifying the First Process

Combustion is a chemical process that one can determine an enthalpy change for. It is an oxidation process where a substance reacts rapidly with oxygen and gives off heat. This reaction is exothermic and the enthalpy change can be calculated knowing the initial and final states.
02

Identifying the Second Process

Phase change or phase transition is another type of process where enthalpy change can be determined. An example of this is the melting of ice into water. The energy required to accomplish this without altering the temperature is known as the enthalpy of fusion. Furthermore, the change in enthalpy for phase transitions can be calculated using the heat of transformation.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Combustion
Combustion is a chemical process involving the rapid reaction of a substance with oxygen. This reaction releases energy in the form of heat and light. It's a perfect example of an exothermic reaction, meaning it releases heat into the surroundings.
  • During combustion, bonds in the reactants (such as hydrocarbons) break, and new bonds form in the products (usually carbon dioxide and water).
  • The released energy during this transition contributes to the heat we observe.
To calculate the enthalpy change during combustion, we measure the difference in enthalpies between the reactants and the products. The enthalpy of combustion can be determined using calorimetry, where the heat evolution for a known amount of reactant is measured.
Phase Change
Phase change, also known as phase transition, occurs when a substance changes from one state of matter to another, such as solid to liquid or liquid to gas. These changes are accompanied by energy transitions but not temperature changes.
  • Common phase changes include melting, freezing, vaporization, and condensation.
  • During a phase change, energy is absorbed or released to facilitate the transition between phases.
While the temperature remains constant during phase changes, the energy change is linked to the enthalpy of the transformation process, which can be computed through calorimetric measurements.
Exothermic Reaction
An exothermic reaction is a type of reaction that releases energy into the surroundings, often in the form of heat. Combustion, as mentioned earlier, is a typical example.
  • In exothermic reactions, the energy of the products is lower than that of the reactants.
  • This difference in energy results in the release of energy, often making the surroundings hotter.
Exothermic reactions are crucial in many natural processes and industrial applications, such as engine performance and heat generation. It鈥檚 essential to understand these reactions to harness their energy effectively.
Enthalpy of Fusion
Enthalpy of fusion is the energy needed to change a substance from a solid to a liquid at its melting point. It鈥檚 an important concept in thermodynamics, reflecting the energy required to overcome intermolecular forces within a solid.
  • It is expressed as the amount of energy per mole or kilogram needed to change from solid to liquid without temperature change.
  • This is crucial for understanding processes like melting ice or metals.
The enthalpy of fusion is determined using calorimetric methods, by calculating the energy absorbed as a solid melts at a constant temperature. This concept helps in understanding energy changes during phase transitions.

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Most popular questions from this chapter

Given the entropy change for the first two reactions below, calculate the entropy change for the third reaction below. \begin{equation} \begin{array}{c}{\mathrm{S}_{8}(s)+8 \mathrm{O}_{2}(g) \rightarrow 8 \mathrm{SO}_{2}(g) \Delta S=89 \mathrm{J} / \mathrm{K}} \\ {2 \mathrm{SO}_{2}(s)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{SO}_{3}(g) \Delta S=-188 \mathrm{J} / \mathrm{K}} \\ {\mathrm{S}_{8}(s)+12 \mathrm{O}_{2}(g) \rightarrow 8 \mathrm{SO}_{3}(g) \Delta S=?}\end{array} \end{equation}

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