{"id":315169,"date":"2023-04-12T10:59:15","date_gmt":"2023-04-12T03:59:15","guid":{"rendered":"https:\/\/quipperhome.wpcomstaging.com\/?p=315169"},"modified":"2023-04-12T10:59:24","modified_gmt":"2023-04-12T03:59:24","slug":"hukum-faraday","status":"publish","type":"post","link":"https:\/\/quipperhome.wpcomstaging.com\/mapel\/kimia\/hukum-faraday\/","title":{"rendered":"Hukum Faraday: Pengertian, Bunyi, Rumus, dan Contoh Soalnya"},"content":{"rendered":"\n<figure class=\"wp-block-image size-full\"><img fetchpriority=\"high\" decoding=\"async\" width=\"1526\" height=\"1002\" src=\"https:\/\/quipperhome.wpcomstaging.com\/wp-content\/uploads\/2023\/04\/Hukum-Faraday-Pengertian-Bunyi-Rumus-dan-Contoh-Soalnya.webp\" alt=\"Hukum Faraday Pengertian, Bunyi, Rumus, dan Contoh Soalnya\" class=\"wp-image-315194\" srcset=\"https:\/\/quipperhome.wpcomstaging.com\/wp-content\/uploads\/2023\/04\/Hukum-Faraday-Pengertian-Bunyi-Rumus-dan-Contoh-Soalnya.webp 1526w, https:\/\/quipperhome.wpcomstaging.com\/wp-content\/uploads\/2023\/04\/Hukum-Faraday-Pengertian-Bunyi-Rumus-dan-Contoh-Soalnya-768x504.webp 768w, https:\/\/quipperhome.wpcomstaging.com\/wp-content\/uploads\/2023\/04\/Hukum-Faraday-Pengertian-Bunyi-Rumus-dan-Contoh-Soalnya-1200x788.webp 1200w, https:\/\/quipperhome.wpcomstaging.com\/wp-content\/uploads\/2023\/04\/Hukum-Faraday-Pengertian-Bunyi-Rumus-dan-Contoh-Soalnya-1170x768.webp 1170w\" sizes=\"(max-width: 1526px) 100vw, 1526px\" \/><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">Quipperian, apakah saat ini kamu sedang belajar tentang <a href=\"https:\/\/www.quipper.com\/id\/blog\/mapel\/kimia\/perbedaan-sel-volta-dan-sel-elektrolisis\/\">sel elektrolisis<\/a>? Kalau begitu, kamu tentu sudah tidak asing lagi, ya dengan hukum Faraday karena hukum ini berkaitan erat dengan sel elektrolisis.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Hukum Faraday adalah sebuah hukum yang ditemukan oleh Michael Faraday, seorang ahli kimia dan fisika asal Inggris. Hukum ini tidak hanya digunakan dalam ilmu Kimia saja, tapi juga ilmu Fisika.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Lalu, seperti apa bunyi hukum Faraday ini? Bagaimana rumusnya? Yuk, simak pembahasan lengkapnya berikut ini.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">Pengertian Hukum Faraday<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">Hukum Faraday adalah hukum yang menjelaskan tentang hubungan antara jumlah listrik yang digunakan dengan massa zat yang dihasilkan, baik di katode maupun anode pada proses elektrolisis. Hukum ini ditemukan oleh Michael Faraday, seorang ahli kimia dan fisika asal Inggris pada tahun 1834. Itulah mengapa, hukum ini dinamakan hukum Faraday, sesuai dengan nama penemunya.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Hukum Faraday ini menjadi salah satu hukum yang memiliki sumbangsih yang besar terhadap kemajuan listrik. Hukum ini juga tidak hanya digunakan dalam ilmu Kimia saja, tapi juga ilmu Fisika. Oleh karena itu, ketika kamu mempelajari mata pelajaran Fisika, kamu mungkin akan menemukan hukum ini.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">Bunyi Hukum Faraday<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">Hukum Faraday dibagi menjadi dua, yaitu hukum Faraday 1 dan hukum Faraday 2. Berikut bunyi hukum Faraday 1:<\/p>\n\n\n\n<p class=\"has-text-align-center wp-block-paragraph\"><strong>\u201cMassa zat yang dilepaskan selama elektrolisis berbanding lurus dengan jumlah listrik yang digunakan\u201d<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Sementara itu, hukum Faraday 2 berbunyi:<\/p>\n\n\n\n<p class=\"has-text-align-center wp-block-paragraph\"><strong>\u201cMassa zat yang dilepaskan pada elektrolisis berbanding lurus dengan massa ekuivalen zat itu\u201d<\/strong><\/p>\n\n\n\n<h2 class=\"wp-block-heading\">Sejarah Hukum Faraday<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">Penemuan hukum Faraday bermula pada saat Michael Faraday berhasil menemukan pengaruh elektromagnetik di tahun 1831. Penemuannya ini dianggap sebagai penemuan monumental karena memiliki artian penting dalam pengertian teoritis tentang elektromagnetik yang dapat digunakan untuk sebagai penggerak arus listrik secara terus-menerus seperti yang diperagakan oleh Michael Faraday sendiri.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Setelah menemukan elektromagnetik, ilmuwan asal Inggris ini melakukan percobaan di bidang Kimia. Faraday akhirnya menemukan adanya hubungan antara jumlah listrik yang digunakan dengan massa zat yang dihasilkan, baik di katode maupun anode pada proses elektrolisis pada tahun 1834. Fakta hubungan tersebut kemudian oleh Faraday disimpulkan sebagai hukum Faraday.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Tak hanya itu saja, Michael Faraday juga menemukan dua hukum elektrolisis yang menjadi dasar elektrokimia, yaitu hukum Faraday 1 dan hukum Faraday 2. Faraday juga banyak mempopulerkan istilah-istilah kimia, seperti elektroda, elektrolit, anoda, katoda, dan sebagainya. Kini, hukum Faraday banyak digunakan secara luas pada berbagai bidang industri.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">Rumus Hukum Faraday<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">Selain memiliki bunyi yang berbeda, hukum Faraday 1 dan 2 juga memiliki rumus yang berbeda. Adapun rumus hukum Faraday 1 dan 2 adalah sebagai berikut.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Rumus Hukum Faraday 1<\/h3>\n\n\n\n<p class=\"wp-block-paragraph\">Ingat, bunyi hukum Faraday 1:<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><em><strong>\u201cMassa zat yang dilepaskan selama elektrolisis berbanding lurus dengan jumlah listrik yang digunakan\u201d<\/strong><\/em><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Berdasarkan bunyinya, rumus hukum Faraday 1 dapat dituliskan sebagai berikut.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>G \u2248 Q atau G \u2248 it<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Keterangan:<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">G = massa yang dihasilkan pada elektrolisis (gram)<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">i = arus listrik (ampere)<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">t = waktu (detik)<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Q = muatan listrik dalam sel (Coulomb)<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Rumus Hukum Faraday 2<\/h3>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>\u201cMassa zat yang dilepaskan pada elektrolisis berbanding lurus dengan massa ekuivalen zat itu\u201d<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Berdasarkan bunyi hukum Faraday 2 tersebut, maka rumusnya adalah:<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" width=\"191\" height=\"55\" src=\"https:\/\/quipperhome.wpcomstaging.com\/wp-content\/uploads\/2023\/04\/Rumus-Hukum-Faraday-2.png\" alt=\"\" class=\"wp-image-315174\"\/><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">Keterangan:<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">ME = massa ekivalen<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">x = jumlah elektron yang diterima atau dilepaskan<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Jika rumus hukum Faraday 1 dan 2 ini digabungkan, maka akan diperoleh rumus baru, yaitu:<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>G = k . i . t . ME<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Keterangan:<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">k = tetapan\/faktor pembanding<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Faraday menemukan bahwa harga faktor pembanding ini adalah 1\/96.500, sehingga rumus di atas dapat dituliskan sebagai berikut.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" width=\"143\" height=\"58\" src=\"https:\/\/quipperhome.wpcomstaging.com\/wp-content\/uploads\/2023\/04\/Faraday-menemukan-bahwa-harga-faktor-pembanding-ini-adalah-196.500.png\" alt=\"Faraday menemukan bahwa harga faktor pembanding ini adalah 196.500\" class=\"wp-image-315177\"\/><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">di mana :<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">G = massa yang dihasilkan pada elektrolisis (gram)<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">i = arus listrik (ampere)<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">t = waktu (detik)<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">ME = massa ekivalen<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Ar = massa atom relatif<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">x = jumlah elektron yang diterima atau dilepaskan<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">Penerapan Hukum Faraday<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">Hukum Faraday banyak digunakan dalam berbagai bidang industri. Berikut adalah beberapa contoh penerapan hukum yang ditemukan oleh Michael Faraday ini dalam kehidupan sehari-hari.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Produksi Zat atau Bahan-bahan Kimia<\/h3>\n\n\n\n<p class=\"wp-block-paragraph\">Zat atau bahan-bahan kimia yang sering digunakan dalam industri, laboratorium, maupun dalam kehidupan sehari-hari ternyata banyak dihasilkan melalui proses elektrolisis. Contohnya, pembuatan gas oksigen, hidrogen, atau gas klorin di laboratorium.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Pemurnian Logam Kotor<\/h3>\n\n\n\n<p class=\"wp-block-paragraph\">Penerapan hukum Faraday berikutnya adalah pada proses pemurnian logam kotor. Pemurnian logam ini dilakukan dengan cara elektrolisis.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Caranya adalah dengan menyusun logam kotor sebagai anode dan logam murni sebagai katode dalam larutan C<sub>u<\/sub>SO<sub>4<\/sub> sebagai larutan elektrolitnya. Dari proses pemurnian logam kotor ini akan menghasilkan logam tunggal murni.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Penyepuhan Logam<\/h3>\n\n\n\n<p class=\"wp-block-paragraph\">Penyepuhan adalah pelapisan logam dengan logam lainnya melalui proses elektrolisis. Tujuannya adalah untuk melindungi logam tersebut dari korosi sekaligus memperindah penampilan logam. Contohnya, penyepuhan alat-alat makan dengan perak atau emas.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">Contoh Soal Hukum Faraday dan Pembahasannya<\/h2>\n\n\n\n<p class=\"wp-block-paragraph\">Kalau tadi penerapan hukum Faraday dalam kehidupan sehari-hari, bagaimana penerapan hukum tersebut dalam soal? Berikut adalah beberapa contoh soal dan pembahasannya untuk membantu kamu memahami hukum Faraday ini.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Contoh 1<\/h3>\n\n\n\n<p class=\"wp-block-paragraph\">Hitunglah massa tembaga yang dihasilkan jika arus listrik sebesar 10 ampere dialirkan selama 9.500 detik ke dalam larutan C<sub>u<\/sub>SO<sub>4<\/sub> (Ar Cu= 63,5)!<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Pembahasan<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Reaksi pengendapan Cu:<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Cu<sup>2+<\/sup><sub>(aq)<\/sub> + 2e \u2192 Cu<sub>(s)<\/sub><\/p>\n\n\n\n<figure class=\"wp-block-image size-full is-resized\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/quipperhome.wpcomstaging.com\/wp-content\/uploads\/2023\/04\/soal-1.png\" alt=\"\" class=\"wp-image-315181\" width=\"191\" height=\"38\"\/><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">Maka, massa Cu yang dihasilkan adalah:<\/p>\n\n\n\n<figure class=\"wp-block-image size-full is-resized\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/quipperhome.wpcomstaging.com\/wp-content\/uploads\/2023\/04\/hasil-soal-1-hukum-faraday.png\" alt=\"\" class=\"wp-image-315182\" width=\"170\" height=\"116\"\/><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">Jadi, massa tembaga yang dihasilkan adalah sebesar 31,75 gram.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Contoh 2<\/h3>\n\n\n\n<p class=\"wp-block-paragraph\">Berapa emas dan klor yang terbentuk, jika arus listrik 10 A melewati larutan emas(III) klorida selama 6 menit? (Ar Au = 196,73; Ar Cl = 35,45). Diketahui reaksi pada elektrode:<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Katode: Au3+(aq) + 3e\u2013 \u2192 Au(s)<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Anode: 2Cl\u2013 (aq) \u2192 Cl2(g) + 2e\u2013<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Pembahasan<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Massa ekuivalen Au adalah 196,73 \/ 3 = 65,66 gram<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Massa ekuivalen Cl<sub>2 <\/sub>adalah 35,45 \/ 1 = 35,45 gram<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Au yang terbentuk<\/p>\n\n\n\n<figure class=\"wp-block-image size-full is-resized\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/quipperhome.wpcomstaging.com\/wp-content\/uploads\/2023\/04\/Au-yang-terbentuk.png\" alt=\"\" class=\"wp-image-315186\" width=\"115\" height=\"110\"\/><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">Cl<sub>2<\/sub> yang terbentuk<\/p>\n\n\n\n<figure class=\"wp-block-image size-full is-resized\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/quipperhome.wpcomstaging.com\/wp-content\/uploads\/2023\/04\/Cl2-yang-terbentuk-.png\" alt=\"\" class=\"wp-image-315187\" width=\"118\" height=\"114\"\/><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">Jadi, emas yang terbentuk adalah 2,45 gram, sedangkan klor yang terbentuk adalah 1,32 gram.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Contoh 3<\/h3>\n\n\n\n<p class=\"wp-block-paragraph\">Berapa waktu yang diperlukan untuk mengendapkan 5,60 gram besi dalam larutan besi (III) klorida dengan arus 5 A? (Ar Fe = 55,85). Diketahui reaksi pada katode:<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Fe<sup>3+<\/sup><sub>(aq)<\/sub> + 3e<sup>\u2013<\/sup> \u2192 Fe<sub>(s)<\/sub><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Massa ekuivalen Fe adalah 55,85 \/ 3 = 18,62 gram<\/p>\n\n\n\n<figure class=\"wp-block-image size-full is-resized\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/quipperhome.wpcomstaging.com\/wp-content\/uploads\/2023\/04\/jawaban-soal-3-hukum-faraday.png\" alt=\"\" class=\"wp-image-315190\" width=\"204\" height=\"117\"\/><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">Jadi, waktu yang diperlukan untuk mengendapkan 5,60 gram besi dalam larutan besi (III) klorida dengan arus 5 A adalah 5.804 detik.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Itu dia pembahasan mengenai hukum Faraday dalam mata pelajaran Kimia. Agar kamu semakin paham dengan hukum ini, cobalah untuk sering mengerjakan soal latihannya, ya. Sampai jumpa di pembahasan Quipper Blog berikutnya<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Sumber :<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Partana, Crys Fajar, dan Antuni Wiyarsi. 2009. Mari Belajar Kimia 3 : Untuk SMA-MA Kelas XII IPA. Jakarta : Pusat Perbukuan, Departemen Pendidikan Nasional<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Pangajuanto, Teguh dan Tri Rahmidi. 2009. Kimia 3: Untuk SMA\/MA Kelas XII. Jakarta: Pusat Perbukuan Departemen Pendidikan Nasional<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Salirawati, Das, dkk. 2007. Belajar Kimia Secara Menarik untuk SMA\/MA Kelas XII. Jakarta: Grasindo<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Sarwosri, Tri. 2017. Tokoh Dunia Sains. Sukoharjo: Penerbit Panembahan Senopati<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Quipperian, apakah saat ini kamu sedang belajar tentang sel elektrolisis? Kalau begitu, kamu tentu sudah tidak asing lagi, ya dengan hukum Faraday karena hukum&hellip;<\/p>\n","protected":false},"author":156742505,"featured_media":315194,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"_crdt_document":"","_monsterinsights_skip_tracking":false,"_monsterinsights_sitenote_active":false,"_monsterinsights_sitenote_note":"","_monsterinsights_sitenote_category":0,"_jetpack_memberships_contains_paid_content":false,"footnotes":""},"categories":[679384879],"tags":[],"ppma_author":[679386846,679386839],"class_list":["post-315169","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-kimia"],"acf":[],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v27.5 - https:\/\/yoast.com\/product\/yoast-seo-wordpress\/ -->\n<title>Hukum Faraday: Pengertian, Bunyi, Rumus, dan Contoh Soalnya - Quipper Blog<\/title>\n<meta name=\"description\" content=\"Hukum Faraday adalah hukum yang ditemukan oleh Michael Faraday. 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