11-9 - Separate the following net redox rxn into half rxns...

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Separate the following net redox rxn into half rxns Cu 2+   (aq) + 2e-   Cu(s) Fe(s) +   Fe 2+  (aq) + 2e- Reduction 1/2 rxn Oxidation 1/2 rxn Fe(s)  +  Cu 2+   (aq)     Cu(s)   +   Fe 2+  (aq)  Orbital E Fe(s) Cu 2+ Fe 2+ Cu(s) Section 11.3 Where did the energy go that was given off?
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Galvanic cell:  Electrochemical cell  in which electrons transfer spontaneously through an external circuit. chemical energy                      electrical energy                      converted into ( ) Cu 2+  (aq) + 2e-  Cu(s) Reduction compartment Cu Cu2+ Fe(s) +   Fe 2+  (aq) + 2e- Fe Fe 2+ Oxidation compartment Liquid junction Potential - + Orbital E Fe(s) Cu 2+ Hi Lo Section 11.3
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V Galvanic cell:  Electrochemical cell  Cu 2+  (aq) + 2e-  Cu(s) Fe(s) +   Fe 2+  (aq) + 2e- Cu Fe Reduction compartment Oxidation compartment anode cathode Orbital E Fe(s) Cu 2+ Potential - + Hi Lo e e e e   Salt bridge K Cl Fe 2+ Cu2+ K Section 11.3
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Galvanic cell:  Electrochemical cell   Cu(s) Fe(s) +   Fe 2+  (aq) + 2e- Fe Fe 2+ Reduction compartment Oxidation compartment Liquid junction anode e Cl K Section 11.3
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V cat an e e e e E cell  =  E cat  -  E an E = E E = E f - E - E i E cell  = E cell  = + 0.78V E cell  > 0 G = - E If  E  > 0, then  G < 0   = + 0.78V – (-0.44V)   +0.34V Section 11.3 Cu Cu2+ Fe Fe 2+
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Orbital energy Electrical potential (voltage) lo hi hi lo Cu 2+  (aq) + 2e-  Cu(s) +0.34 V  Section 11.4 Standard Reduction Potentials E cell  = = + 0.78V – (-0.44V)   +0.34V
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E cell  =  E cat  -  E an Section 11.3 e e e e Electrons don’t care how YOU hook the leads up -V an cat In lab, the voltmeter was hooked up backward for some examples.  The voltage read negative.
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11-9 - Separate the following net redox rxn into half rxns...

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