🧪 Chemistry Quiz 20: Electrochemistry and Batteries

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🧪 Chemistry · Quiz 020

Convert CHEM-019 redox bookkeeping into spatially separated half-reactions that produce or consume electrical work in electrochemical cells and batteries.

Learning goalAnalyze anode-cathode roles, electron and ion movement, standard cell potential, salt-bridge function, and rechargeable battery energy conversion.

  • 5 questions
  • Advanced connections
  • Explanations after finishing
Answered 0/5
FoundationWhich electrode statement is always correct by electrochemical definition?
Need a small nudge?

Electrode names are tied to reaction type, whereas electrode signs depend on whether the cell is galvanic or electrolytic.

UnderstandingIn a working galvanic cell, in which direction do electrons travel through the external metallic circuit?
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Electrons are produced where oxidation occurs and consumed where reduction occurs.

ApplicationA Zn-Cu galvanic cell uses the standard reduction potentials E°(Cu²⁺/Cu) = +0.34 V and E°(Zn²⁺/Zn) = −0.76 V. If Cu is the cathode and Zn the anode, what is E°cell?
Need a small nudge?

Use E°cell = E°cathode − E°anode with both tabulated values written as reduction potentials.

InterpretationWhat is the primary role of a salt bridge in a conventional galvanic cell?
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Without the bridge, ask what electrical imbalance would develop in each half-cell as oxidation and reduction continue.

ConnectionWhich statement best describes energy conversion in a rechargeable battery over discharge and charging?
Need a small nudge?

Treat discharge as the battery powering a circuit and charging as an external source forcing the chemistry back toward a higher-energy stored state.

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