penentuan entalpi reaksi fix tanpa video
TRANSCRIPT
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Media pendidikan
Dra. Hj. Atiek Winarti, M.Pd, M.Sc
Drs. H. M. Kusasi, M.Pd
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SK: Memahami perubahan energi
dalam reaksi kimia dan cara
pengukurannya
KD : Perubahan entalpi
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KALORIMETRI
HUKUM HESS
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GAMBAR
FLASH
VIDEO
PENJELASAN
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Suatu sistem terisolasi (tidak ada pertukaran materi maupun energi dengan
lingkungan di luar kalorimetri)
qair = m x c x ∆T
qbom = C x ∆T
qreaksi = - (qair + qbom)
∆H = q
qreaksi = - qlarutan
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Sebanyak 50 mL larutan HCl 0.1 M dicampurdengan 50 mL larutan NaOH 0.1 M. Ternyata suhularutan naik sekitar 3oC. Apabila larutan mempunyaikerapatan 1 g/mL dan c larutan 4.2 J/g oC. Tentukankalor reaksinya.
HCl + NaOH NaCl + H2O
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• Jawab:
Dikeahui:
V HCl : 50 mL , M HCl = 0.1 mol/ L
V NaOH : 50 ml, M NaOH = 0.1 mol/L
∆T = 3 oC
ρ = 1 g/mL
c = 4.2 J/g oC
Ditanya:
q reaksi = .....?
q reaksi = m x c x ∆T
= (100 mL x 1 g/mL) x
4.2 J/g oC x 3 oC
= 1260 J
= 1.26 kJ
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VIDEO
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Diagram 1 dan 2
Flash
Video
Penjelasan
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“ kalor reaksi hanya bergantung pada keadaan awal dan keadaan akhir, tidak pada lintasan”
Ada 3 cara mengitung
entalpi yang dilandaskan atas hukum
hess
1. Data entalpi standar (∆Ho
f )
2. Diagram siklus
3. Energi ikatan
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Berdasarkan hukum hess
Contoh:
H2(g) + F2(g) 2HF(g) ∆H =-537 kJC(s) + 2F2(g) CF2(g) ∆H = -680 kJ2C(s) + 2H2(g) C2H4(g) ∆H = 52.3 kJ
Jawab :
2H2(g) + 2F2(g) 4HF(g) ∆H =-1074 kJ2C(s) + 4F2(g) 2CF4(g) ∆H = -1360 kJC2H4(g) 2C(s) + 2H2(g) ∆H = -52.3 kJ
C2H4(g) + 6F2(g) 2CF4(g) + 4HF(g) ∆H =-2486.3 kJ
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1. Berdasarkan data entalpi pembentukan standar (∆Hof )
∆Hreaksi = ∑ n ∆Hof produk - ∑ m ∆Ho
f reaktan
Contoh:
Diketahui entalpi pembetukan metanol, CH4O(l) = -238.6 kJ ; CO2(g)
= -393.5 kJ ; H2O(l) = -286 kJ. Tentukan entalpi pembakaran metanol membentuk gas CO2(g) dan air
Reaksi:CH4O(l) + 3/2 O2(g) CO2(g) + 2H2O(l) ∆H = ???
∆H0 = [∆H0f CO2(g) + 2 x ∆H0
f 2H2O(l) ] – [∆H0f CH4O(l) + 3/2 x ∆H0
f O2(g)
∆H0 = [-393.5 kJ + 2 x (-286 kJ)] – 238.6 kJ + 3/2 x 0 kJ]∆H0 = -726.9 kJ
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2. BERDASARKAN DIAGRAM SIKLUS
(DIAGRAM TINGKAT ENERGI)
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1. Energi atomisasi
CH4 C + 4H ∆H= 1668 kJ
CH4 memiliki 4 ikatan C-H, dan energi ikatan C-H = 417 kJ maka energi atomisasi CH4 = 4 x 417 kJ = 1668 kJ
3. Berdasarkan energi ikatan
2. Energi disosiasi ikatan
CH4 CH3 + H ∆H= 431 kJ
Energi ikatan untuk memutuskan 1 atom H dari olekul CH4 sebesar 431 kJ
3. Energi ikatan rata-rata (D)
∆H = ∑Epemutusan reaktan - ∑Epenggabungan produk
CH4 C + 4H ∆H= 1668 kJ
Energi ikatan rata-rata C-H (DC-H ) = 1668/4 = 417 kJ
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VIDEO
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http://uyararjunlhuka.blogspot.com/
Daftar pustaka:
Purba, Michael. 2006. Kimia untuk
SMA kelas XI. Jakarta: Erangga
Rufaida, Anis Dyah. 2009. Kimia
untuk SMA/MA kelas XI semsester 1.
Klaten: Intan Pariwara
Kunjungi BLOG saya
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