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TERMOKIMIA

TERMOKIMIA. STANDAR KOMPETENSI. Memahami perubahan energi dalam reaksi kimia dan cara pengukurannya. KOMPETENSI DASAR. Mendeskripsikan perubahan entalpi suatu reaksi, reaksi eksoterm, dan reaksi endoterm. Indikator. Menjelaskan hukum/azas kekekalan energi Membedakan sistem dan lingkungan

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TERMOKIMIA

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  1. TERMOKIMIA

  2. STANDAR KOMPETENSI Memahami perubahan energi dalam reaksi kimia dan cara pengukurannya.

  3. KOMPETENSI DASAR Mendeskripsikan perubahan entalpi suatu reaksi, reaksi eksoterm, dan reaksi endoterm.

  4. Indikator • Menjelaskan hukum/azas kekekalan energi • Membedakan sistem dan lingkungan • Membedakan reaksi eksoterm dan endoterm melalui percobaan • Menjelaskan macam-macam perubahan entalpi

  5. AZAS KEKEKALAN ENERGI

  6. 1. Sistem dan Lingkungan • Sistem • Lingkungan • Sistem terbuka • Sistem tertutup • Sistem terisolasi

  7. b a c

  8. 2. Energi Dalam (E) • Energi kinetik • Energi potensial • Energi dalam • Energi termal • Energi kimia

  9. didinginkan 1 mol air, 100ºC, 1atm 1 mol air, 25ºC, 1atm E = p kJ E = x kJ dipanaskan 1 mol air, 0ºC, 1atm 1 mol air, 25ºC, 1atm E = q kJ E = y kJ p > q x = y

  10. E = E2 – E1 • E = Ep – Er • Ep > Er  E = Ep – Er > 0 • Ep < Er  E = Ep – Er < 0

  11. 3. Kerja (w) • w = F x s • F = P x A • w = F x h = P x A x h = P x V • 1 L.atm = 101,32 J P A h P P A gas gas

  12. 4. Kalor (q) • q = m c t • q = C t

  13. 5. Hukum Pertama Termodinamika (Azas Kekekalan Energi) • Energi dapat diubah tetapi tidak dapat dimusnahkan atau diciptakan. • E = q + w • Sistem menerima kalor, q bertanda + • Sistem membebaskan kalor, q bertanda – • Sistem melakukan kerja, w bertanda – • Sistem menerima kerja, w bertanda +

  14. lingkungan +w -w sistem +q -q lingkungan

  15. 6. Kalor Reaksi: E dan H pereaksi pereaksi (keadaan 1) (keadaan 2) E = q + w E1 E2 E = qv + 0 = qv = qreaksi E = qp + w atau qp = E – w = qreaksi

  16. H = qreaksi qreaksi = H = E H = Hp - Hr

  17. 7. Reaksi Eksoterm dan Endoterm kalor kalor kalor kalor sistem sistem kalor lingkungan kalor kalor kalor eksoterm endoterm

  18. Reaksi Endoterm: H = Hp – Hr > 0 Reaksi Eksoterm: H = Hp – Hr < 0

  19. H H P R R P P R R P Reaksi Endoterm: H = Hp – Hr > 0 Reaksi Eksoterm: H = Hp – Hr < 0

  20. 8. Persamaan Termokimia • H2(g) + 1/2O2(g) H2O(l)H= -286 kJ • 2H2(g) + O2(g) 2H2O(l)H= -572 kJ • NH3(g) 1/2N2(g) + 3/2H2(g)H= +46 kJ • 2NH3(g) N2(g) + 3H2(g)H= +92 kJ

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