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Chapter 7: Problem 9

What is the law of conservation of energy?

Short Answer

Expert verified
The law of conservation of energy states that energy cannot be created or destroyed; it can only change forms.

Step by step solution

01

Understand the Concept

The law of conservation of energy states that energy cannot be created or destroyed in an isolated system. It implies that the total energy of an isolated system remains constant over time.
02

Identifying Energy Transformations

Energy can be transformed from one form to another (e.g., potential energy to kinetic energy), but the total amount of energy remains the same in the system. This means that although energy might change its form, the total sum remains constant.
03

Applying in Practical Situations

In practical scenarios, when observing an isolated system, the initial total energy is equal to the final total energy, after all transformations are accounted for. For example, when a ball is dropped, its potential energy is converted into kinetic energy as it falls.

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Key Concepts

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

Energy Transformation
Energy transformation is a fundamental concept governed by the law of conservation of energy. In an isolated system, energy is never lost but simply changes forms. This means energy can transition from potential energy to kinetic energy or vice versa.

Consider a roller coaster at the top of a hill. Initially, the roller coaster has maximum potential energy because of its height. As it begins its descent, this energy transforms into kinetic energy as the roller coaster speeds up.

It is important to remember:
  • The total energy in the system remains constant throughout the transformation.
  • Energy transformations allow energy to perform work, like moving an object or heating a space.
Understanding energy transformations provides insight into how we can harness and utilize energy effectively in various applications.
Isolated System
An isolated system is a critical concept to understand when discussing energy conservation. In physics, an isolated system is characterized by having no exchange of energy or matter with its surroundings. This ideal scenario allows us to ensure that the total energy within the system remains constant over time.

For example, consider a perfectly sealed thermos bottle containing hot soup. Ideally, it's an isolated system because no heat escapes or enters the thermos.
  • Within an isolated system, energy cannot be created or destroyed.
  • Only transformations between different types of energy can occur within the system itself.
This concept is crucial in theoretical physics to simplify and solve problems concerning energy dynamics and helps illustrate purity in energy transformation scenarios.
Potential Energy to Kinetic Energy
The transition from potential energy to kinetic energy is a classic example of energy transformation in action. Potential energy is the stored energy of an object due to its position, like an apple hanging on a tree.

As the apple falls, gravitational force acts on it, and the potential energy is converted into kinetic energy, which powers its downward motion. When the apple reaches the ground, its potential energy is minimized, and its kinetic energy is maximized just before impact.

Here are key points to note:
  • Potential energy is highest at the object's highest point.
  • Kinetic energy increases as the object decreases in height.
  • Total energy remains the same; it's just shifted from one form to another.
This process is perfectly explained by the law of conservation of energy within an isolated system, reaffirming that energy forms may change, but total energy does not.

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Most popular questions from this chapter

Nitrogen gas reacts with oxygen gas to make \(\mathrm{NO}(\mathrm{g})\) while absorbing \(180 \mathrm{~kJ}\). Is this process exothermic or endothermic?

Define formation reaction and give an example.

What does Hess's law require us to do to the \(\Delta H\) of a thermochemical equation if we reverse the equation?

Solid sodium reacts with chlorine gas to make solid sodium chloride while giving off \(772 \mathrm{~kJ}\). Write a properly balanced thermochemical equation for this process.

The \(\Delta H\) for \(\mathrm{C}_{2} \mathrm{H}_{4}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) is \(-44 \mathrm{~kJ}\). What is the \(\Delta H\) for this reaction? \(2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH} \rightarrow 2 \mathrm{C}_{2} \mathrm{H}_{4}+2 \mathrm{H}_{2} \mathrm{O}\)
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