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Elechtrochemistry 17. F = (6.022 x 10 23 mol -1 ) x (1.602192 x 10 -19 C) = 96,484 C mol -1 How much? – Faraday’s constant.

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Presentation on theme: "Elechtrochemistry 17. F = (6.022 x 10 23 mol -1 ) x (1.602192 x 10 -19 C) = 96,484 C mol -1 How much? – Faraday’s constant."— Presentation transcript:

1 Elechtrochemistry 17

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3 F = (6.022 x mol -1 ) x ( x C) = 96,484 C mol -1 How much? – Faraday’s constant.

4 Faraday

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6 Electricity Current = Charge/time - I = Q/t [Ampere]=[Coulomb]/[sec] Potential = Current x Resistance - E = I R (Ohms law) [Volt]=[Ampere] [Ohm]

7 So what is resistance? NB: Potential is relative!

8 Work = Potential x Charge - W = E q [Joule] = [Volt] [Coulomb]

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17 NERNST EQUATION

18 At 25 o C

19 NERNST EQUATION Walther Hermann Nernst 1864–1941

20 NERNST EQUATION

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22 THERMODYNAMICS and equilibrium

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24 NERNST EQUATION

25 0.50 M AgNO3(aq) M Cd(NO3)2(aq)

26 0.50 M AgNO3(aq) M Cd(NO3)2(aq)

27 0.50 M AgNO3(aq) M Cd(NO3)2(aq) My way:

28 Ion selective electrode

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35 BUN: 7 to 20 mg/dL CO2 (carbon dioxide): 20 to 29 mmol/L Creatinine: 0.8 to 1.4 mg/dL Glucose: 64 to 128 mg/dL Serum chloride: 101 to 111 mmol/L Serum potassium: 3.7 to 5.2 mEq/L Serum sodium: 136 to 144 mEq/L CHEM-7 is a group of blood tests that provides information about your body's metabolism. The test is commonly called a basic metabolic panel.

36 Ion selective electrode Selectivity And interference

37 NERNST EQUATION Measure E to determine 1 unknown concentration (…..so fix the other concentrations)

38 Reference electrodes

39 My way:

40 Reference electrodes


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