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Oleh YELI GUSTAMI 54986 / 2010 Pend. Kimia RM Dosen Pembimbing Prof. Dr. ELLIZAR JALIUS, M.Pd

Hukum faraday. Oleh YELI GUSTAMI 54986 / 2010 Pend. Kimia RM Dosen Pembimbing Prof. Dr. ELLIZAR JALIUS, M.Pd. SEL ELEKTROKIMIA. SEL VOLTA. SEL ELEKTROLISIS. Energi Listrik  Reaksi Kimia. Katoda (-)  R eaksi reduksi Anoda (+)  Reaksi oksidasi.

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Oleh YELI GUSTAMI 54986 / 2010 Pend. Kimia RM Dosen Pembimbing Prof. Dr. ELLIZAR JALIUS, M.Pd

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  1. Hukum faraday Oleh YELI GUSTAMI 54986 / 2010 Pend. Kimia RM DosenPembimbing Prof. Dr. ELLIZAR JALIUS, M.Pd

  2. SEL ELEKTROKIMIA SEL VOLTA SEL ELEKTROLISIS EnergiListrik Reaksi Kimia

  3. Katoda (-)  Reaksireduksi Anoda (+)  Reaksioksidasi

  4. HubunganKuantitatifantaramassazat yang dibebaskandanganjumlaharuslistrik yang digunakan.??? Michael Faraday Hukum Faraday

  5. Hukum Faraday Massa zat (G) denganjumlahlistrik (Q) Massa zat (G) denganmassaekivalen (ME) Hukum Faraday I Hukum Faraday II

  6. Hukum Faraday I G ≈ Q Q = i x t G = massazat (gram)I = kuatarus ( ampere )t = waktu (detik / sekon) Jadi, G = ix t

  7. Hukum Faraday II ME = Massa EkivalenAr = Atom Relatif G ≈ME ME = Ar / Biloks

  8. PENGGABUNGAN HUKUM FARADAY I DAN II G = k x i x t x ME dimana k = tetapan atau pembanding k = 1/96.500 Jadi :

  9. Contoh Soal Hitunglah massa tembaga yang dapat dibebaskan oleh arus 10 Ampere yang dialirkan selama 965 detik ke dalam larutan CuSO4

  10. Cu yang diendapkan d katode menurut persamaan berikut : Cu+2 (aq) + 2e → Cu (s)

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