Exam 1 Review

Exam 1 Review - Chemistry 6C: Exam 1 Review...

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Chemistry 6C: Exam 1 Review
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Chemistry 6C: Exam 1 Review Oxidizing Agent vs. Reducing Agent Galvanic (voltaic) cell Anode, cathode E ° red E ° cell Electrochemical Series E cell Δ G and K Charge, Current Corrosion Primary vs. secondary baJeries
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Chemistry 6C: Exam 1 Review 1. Recognize redox reactions. 2. Assign oxidation numbers to each atom in a substance. 3. In a redox reaction, identify the species oxidized, the species reduced, the oxidizing agent, and the reducing agent. 4. Balance a redox reaction (by the half-reaction method) in acidic or basic media.
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Chemistry 6C: Exam 1 Review Which of the following reactions is NOT a reduction-oxidation reaction? (a) 2 H 2 O 2 (aq) 2 H 2 O(l) + O 2 (g) (b) 2 NaN 3 (s) 2 Na(s) + 3N 2 (g) (c) 2 Cu + (aq) Cu 2+ (aq) + Cu(s) (d) 2 Na(s) + 2H 2 O(l) 2 NaOH(s) + H 2 (g) (e) NH 3 (g) + H 2 O(l) NH 4 + (aq) + OH - (aq) Explain. Assign oxidation numbers. Indicate species that are reduced, oxidized, reducing agents, and oxidizing agents.
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Chemistry 6C: Exam 1 Review Balance the following skeletal equation (in basic media): P 4 (s) H 2 PO 2 - (aq) + PH 3 (g)
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Chemistry 6C: Exam 1 Review 5. Sketch a galvanic cell, identifying the anode and cathode half-reactions, the sign of each electrode, and the direction of electron and ion flow. 6. Write balanced chemical equations for reactions occurring in a galvanic cell. 7. Write and interpret shorthand notations for galvanic cells. 8. Use a table of standard reduction potentials to calculate standard cell potentials. 9. Use a table of standard reduction potentials to rank substances in order of increasing oxidizing strength or reducing strength (*relative to the SHE standard) and to determine whether a reaction is spontaneous.
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Chemistry 6C: Exam 1 Review 10. Interconvert cell potential and free-energy change for a reaction. 11. Use the Nernst equation to calculate cell potentials for
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Exam 1 Review - Chemistry 6C: Exam 1 Review...

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