This document contains comments about the article Reversible process (thermodynamics) in Wikipedia
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In the last paragraph I explain my own opinion.

### Introduction

The article starts with the following sentence.
In thermodynamics, a reversible process is a process, involving a system and its surroundings, whose direction can be reversed by infinitesimal changes in some properties of the surroundings, such as pressure or temperature.
It should be understood that the surroundings are part of the process. When you heat a process you add energy. The problem is this requires a heating unit as part of the original process.
While processes in isolated systems are never reversible, cyclical processes can be reversible or irreversible.
It is important to understand the difference when.
Reversible processes are hypothetical or idealized but central to the second law of thermodynamics.
It does not make sense to study hypothetical processes.

### 1. Overview

Thermodynamic processes can be carried out in one of two ways: reversibly or irreversibly.
Okay. Let's continue.
An ideal thermodynamically reversible process is free of dissipative losses and therefore the magnitude of work performed by or on the system would be maximized.
The word ideal is mentioned. The reality is different. There are always losses.

### 3. Boundaries and states

Simple reversible processes change the state of a system in such a way that the net change in the combined entropy of the system and its surroundings is zero.
When the surroundings are involved, the whole process becomes more complex.
Nevertheless, the Carnot cycle demonstrates that the state of the surroundings may change in a reversible process as the system returns to its initial state.

### Reflection 1 - Reversible versus irreversible processes

In any (chemical) process a certain reaction takes place. That means two atoms can combine to form a molecule. For example: H2 + CL2 gives 2HCL
But also the reverse can happen HCL gives H2 + CL2. But does that mean that such a process

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Created: 1 November 2022

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