{"id":2609,"date":"2026-05-18T16:48:48","date_gmt":"2026-05-18T07:48:48","guid":{"rendered":"https:\/\/training.contentsda.kr\/?post_type=courses&p=2609"},"modified":"2026-05-18T07:48:49","modified_gmt":"2026-05-18T07:48:49","slug":"galvanic-cell-making-battery","status":"publish","type":"courses","link":"https:\/\/training.contentsda.kr\/ne\/courses\/galvanic-cell-making-battery\/","title":{"rendered":"Galvanic \u0938\u0947\u0932 - \u092c\u094d\u092f\u093e\u091f\u094d\u0930\u0940 \u092c\u0928\u093e\u0909\u0928\u0947"},"content":{"rendered":"

The process of making a battery from zinc and copper with sulfuric acid is commonly known as a “galvanic cell” or “voltaic cell.” This type of battery is also referred to as a “zinc-copper cell” or a “Daniell cell,” named after the 19th-century scientist John Frederic Daniell who first developed it.<\/p>\n

Here’s a brief overview of how a zinc-copper battery works:<\/p>\n

    \n
  1. Components:<\/strong>\n
      \n
    • Anode (Zinc):<\/strong> The zinc metal serves as the anode and undergoes oxidation. In the Daniell cell, zinc is often in the form of a zinc rod or plate.<\/li>\n
    • Cathode (Copper):<\/strong> The copper metal serves as the cathode and undergoes reduction. In the Daniell cell, copper is typically in the form of a copper rod or plate.<\/li>\n
    • Electrolyte:<\/strong> Sulfuric acid (H2SO4) is used as the electrolyte, facilitating the flow of ions between the anode and cathode.<\/li>\n<\/ul>\n<\/li>\n
    • Chemical Reactions:<\/strong>\n
        \n
      • At the Anode (Zinc):<\/strong> Zn\u00a0(s)<\/span><\/span>\u2192<\/span><\/span>Zn<\/span>2+<\/span><\/span><\/span><\/span><\/span><\/span><\/span>(<\/span>a<\/span>q<\/span>)<\/span>+<\/span><\/span>2<\/span>e<\/span>\u2212<\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/li>\n
      • At the Cathode (Copper):<\/strong> Cu<\/span>2+<\/span><\/span><\/span><\/span><\/span><\/span><\/span>(<\/span>a<\/span>q<\/span>)<\/span>+<\/span><\/span>2<\/span>e<\/span>\u2212<\/span><\/span><\/span><\/span><\/span><\/span><\/span>\u2192<\/span><\/span>Cu\u00a0(s)<\/span><\/span><\/span><\/li>\n<\/ul>\n

        The overall reaction is the combination of these two half-reactions:
        \nZn\u00a0(s)<\/span><\/span>+<\/span><\/span>Cu<\/span>2+<\/span><\/span><\/span><\/span><\/span><\/span><\/span>(<\/span>a<\/span>q<\/span>)<\/span>\u2192<\/span><\/span>Zn<\/span>2+<\/span><\/span><\/span><\/span><\/span><\/span><\/span>(<\/span>a<\/span>q<\/span>)<\/span>+<\/span><\/span>Cu\u00a0(s)<\/span><\/span><\/span><\/li>\n

      • Electron Flow:<\/strong> Electrons flow from the zinc anode to the copper cathode through an external circuit, creating an electric current.<\/li>\n
      • Ion Flow:<\/strong> Zinc ions (Zn\u00b2\u207a) move into the electrolyte, while copper ions (Cu\u00b2\u207a) are reduced at the cathode, leading to the transfer of positive charge.<\/li>\n
      • Salt Bridge:<\/strong> To maintain charge neutrality, a salt bridge or other ion-conductive separator is often used to allow the flow of ions between the anode and cathode compartments without directly mixing the electrolytes.<\/li>\n<\/ol>\n

        The Daniell cell produces a direct current (DC) and was historically significant as one of the early examples of a practical battery. However, modern batteries, such as alkaline or lithium-ion batteries, have largely replaced the Daniell cell for many applications due to their improved efficiency and other characteristics.<\/p>","protected":false},"excerpt":{"rendered":"

        The process of making a battery from zinc and copper with sulfuric acid is commonly known as a “galvanic cell” or “voltaic cell.” This type of battery is also referred to as a “zinc-copper cell” or a “Daniell cell,” named after the 19th-century scientist John Frederic Daniell who first developed it. Here’s a brief overview […]<\/p>\n","protected":false},"author":1,"featured_media":3220,"template":"","course-category":[61,60],"course-tag":[],"class_list":["post-2609","courses","type-courses","status-publish","has-post-thumbnail","hentry","course-category-cardboard","course-category-webgl","pmpro-has-access"],"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/training.contentsda.kr\/ne\/wp-json\/wp\/v2\/courses\/2609","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/training.contentsda.kr\/ne\/wp-json\/wp\/v2\/courses"}],"about":[{"href":"https:\/\/training.contentsda.kr\/ne\/wp-json\/wp\/v2\/types\/courses"}],"author":[{"embeddable":true,"href":"https:\/\/training.contentsda.kr\/ne\/wp-json\/wp\/v2\/users\/1"}],"version-history":[{"count":3,"href":"https:\/\/training.contentsda.kr\/ne\/wp-json\/wp\/v2\/courses\/2609\/revisions"}],"predecessor-version":[{"id":2612,"href":"https:\/\/training.contentsda.kr\/ne\/wp-json\/wp\/v2\/courses\/2609\/revisions\/2612"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/training.contentsda.kr\/ne\/wp-json\/wp\/v2\/media\/3220"}],"wp:attachment":[{"href":"https:\/\/training.contentsda.kr\/ne\/wp-json\/wp\/v2\/media?parent=2609"}],"wp:term":[{"taxonomy":"course-category","embeddable":true,"href":"https:\/\/training.contentsda.kr\/ne\/wp-json\/wp\/v2\/course-category?post=2609"},{"taxonomy":"course-tag","embeddable":true,"href":"https:\/\/training.contentsda.kr\/ne\/wp-json\/wp\/v2\/course-tag?post=2609"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}