galvanic cell

简明释义

伽伐尼电池

英英释义

例句

1.In a chemistry lab, students learned how to build a galvanic cell 电池 using copper and zinc electrodes.

在化学实验室，学生们学习了如何使用铜和锌电极构建一个galvanic cell 电池。

2.The galvanic cell 电池 converts chemical energy into electrical energy through redox reactions.

这个galvanic cell 电池通过氧化还原反应将化学能转化为电能。

3.A simple galvanic cell 电池 can be made with a lemon, a copper coin, and a galvanized nail.

一个简单的galvanic cell 电池可以用一个柠檬、一个铜币和一个镀锌钉制作。

4.The voltage produced by a galvanic cell 电池 depends on the materials used for the electrodes.

由galvanic cell 电池产生的电压取决于用于电极的材料。

5.When the galvanic cell 电池 is connected to a circuit, it can power small devices.

当galvanic cell 电池连接到电路时，它可以为小型设备供电。

作文

A galvanic cell is a vital component in the study of electrochemistry, serving as a fundamental example of how chemical energy can be converted into electrical energy. Understanding the principles behind a galvanic cell not only enhances our knowledge of chemistry but also has significant implications for various applications in technology and industry.At its core, a galvanic cell, also known as a voltaic cell, consists of two different electrodes immersed in an electrolyte solution. These electrodes are typically made of dissimilar metals, such as zinc and copper. When these metals are connected by a wire and placed in an electrolyte, a spontaneous redox reaction occurs. This reaction involves the transfer of electrons from one electrode to another, generating an electric current.The electrode where oxidation occurs is called the anode, while the electrode where reduction takes place is referred to as the cathode. In a typical galvanic cell, the anode is usually the metal that is more reactive, which means it loses electrons more readily. For example, in a zinc-copper galvanic cell, zinc serves as the anode, losing electrons and forming zinc ions. Conversely, the copper electrode acts as the cathode, gaining electrons and reducing copper ions from the electrolyte.One of the fascinating aspects of a galvanic cell is its ability to produce electricity without the need for an external power source. This self-sustaining reaction highlights the principles of thermodynamics and electrochemistry, demonstrating how chemical potential energy is transformed into electrical energy. The voltage produced by a galvanic cell depends on the nature of the electrodes and the electrolyte used, which can be calculated using the Nernst equation.The practical applications of galvanic cells are vast and varied. They are commonly found in batteries, which power everything from small electronic devices to electric vehicles. Understanding how galvanic cells function allows engineers and scientists to design more efficient batteries with longer life spans and higher energy densities. Moreover, galvanic cells are also used in corrosion prevention techniques, where they help protect metals from rusting and degradation.In addition to their practical uses, galvanic cells are essential in educational settings. They provide a hands-on approach to learning about electrochemical processes, enabling students to visualize and understand complex concepts. By constructing simple galvanic cells in the laboratory, students can observe firsthand the principles of oxidation and reduction, as well as the flow of electrons through a circuit.In conclusion, the galvanic cell represents a critical concept in both chemistry and physics, illustrating the conversion of chemical energy into electrical energy through spontaneous reactions. Its significance extends beyond the classroom, influencing technological advancements and everyday applications. By studying galvanic cells, we gain insights into the fundamental principles of energy transformation, paving the way for innovations that harness these processes for practical use.

电池是电化学研究中的重要组成部分，作为化学能转化为电能的基本例子。理解电池背后的原理不仅增强了我们对化学的认识，还对技术和工业中的各种应用具有重要意义。在其核心，电池，也称为伏打电池，由两个不同的电极浸没在电解液中组成。这些电极通常由不同的金属制成，如锌和铜。当这些金属通过导线连接并放置在电解液中时，自发的氧还原反应发生。这个反应涉及电子从一个电极转移到另一个电极，产生电流。氧化发生的电极称为阳极，而还原发生的电极被称为阴极。在典型的电池中，阳极通常是更具反应性的金属，这意味着它更容易失去电子。例如，在锌-铜电池中，锌作为阳极，失去电子并形成锌离子。相反，铜电极作为阴极，获得电子并还原电解液中的铜离子。电池的一个迷人之处在于它能够在没有外部电源的情况下产生电力。这种自我维持的反应突显了热力学和电化学的原理，展示了化学势能如何转化为电能。电池所产生的电压取决于所用电极和电解液的性质，可以使用Nernst方程计算。电池的实际应用广泛而多样。它们通常用于电池，为从小型电子设备到电动汽车的所有设备供电。理解电池的功能使工程师和科学家能够设计出更高效、寿命更长、能量密度更高的电池。此外，电池还用于防腐技术，帮助保护金属免受生锈和降解。除了实际用途，电池在教育环境中也是必不可少的。它们提供了一种动手学习电化学过程的方法，使学生能够可视化和理解复杂的概念。通过在实验室中构建简单的电池，学生可以亲眼观察氧化和还原的原理，以及电子在电路中的流动。总之，电池代表了化学和物理中的一个关键概念，说明了通过自发反应将化学能转化为电能。它的重要性超越了课堂，对技术进步和日常应用产生了影响。通过研究电池，我们获得了对能量转化基本原理的深入理解，为利用这些过程的创新铺平了道路。