AP Chemistry Flashcards: Galvanic Voltaic And Electrolytic Cells

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This deck focuses on Galvanic Voltaic And Electrolytic Cells, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

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Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

Flashcard 1: State the relationship between Gibbs free energy and cell potential.

Answer: $\Delta G = -nFE_{cell}$. Links thermodynamic favorability to electrochemical potential.

Flashcard 2: What is the role of a porous disk in a galvanic cell?

Answer: To allow ion exchange while preventing mixing. Similar to salt bridge but uses physical barrier.

Flashcard 3: Find the cell potential given $E_{cathode} = 0.80$ V and $E_{anode} = 0.40$ V.

Answer: $0.40$ V. Using $E_{cell} = E_{cathode} - E_{anode} = 0.80 - 0.40$.

Flashcard 4: What does a positive cell potential indicate?

Answer: The reaction is spontaneous. Reaction proceeds naturally without external energy input.

Flashcard 5: What is the role of the salt bridge in a galvanic cell?

Answer: To maintain electrical neutrality. Allows ion migration to balance charge as reactions proceed.

Flashcard 6: Identify the charge of the anode in a galvanic cell.

Answer: Negative. Loses electrons during oxidation, creating electron excess.

Flashcard 7: Identify the charge of the cathode in a galvanic cell.

Answer: Positive. Gains electrons during reduction, creating electron deficiency.

Flashcard 8: Which metal acts as a reducing agent in a galvanic cell?

Answer: The metal at the anode. Undergoes oxidation, losing electrons to external circuit.

Flashcard 9: What happens to the mass of the cathode in a galvanic cell during operation?

Answer: It increases. Metal ions deposit as reduction occurs.

Flashcard 10: What occurs at the cathode in a galvanic cell?

Answer: Reduction. Electrons are gained, making cathode the electron destination.

Flashcard 11: What occurs at the cathode in a galvanic cell?

Answer: Reduction. Electrons are gained, making cathode the electron destination.

Flashcard 12: What occurs at the anode in a galvanic cell?

Answer: Oxidation. Electrons are lost, making anode the source of electrons.

Flashcard 13: State the direction of electron flow in an electrolytic cell.

Answer: From cathode to anode. External power source forces electrons from cathode to anode.

Flashcard 14: What is a characteristic of a rechargeable battery in terms of cell type?

Answer: Can act as both galvanic and electrolytic cell. Charging and discharging involve opposite spontaneity directions.

Flashcard 15: What is the standard cell potential $(E^\theta)$ for a galvanic cell?

Answer: Positive. Spontaneous reactions have positive cell potentials.

Flashcard 16: State the relationship between Gibbs free energy and cell potential.

Answer: $\Delta G = -nFE_{cell}$. Links thermodynamic favorability to electrochemical potential.

Flashcard 17: What occurs at the cathode in an electrolytic cell?

Answer: Reduction. Reduction still occurs at cathode regardless of cell type.

Flashcard 18: Identify the charge of the anode in an electrolytic cell.

Answer: Positive. Connected to positive terminal of external power source.

Flashcard 19: State the effect of temperature on cell potential.

Answer: Cell potential generally decreases with increasing temperature. Higher temperature typically reduces driving force for reaction.

Flashcard 20: Define Faraday's constant.

Answer: The charge of one mole of electrons, approximately 96485 C/mol. Fundamental constant relating charge to moles of electrons.

Flashcard 21: What is the main difference between galvanic and electrolytic cells?

Answer: Galvanic cells are spontaneous; electrolytic cells are non-spontaneous. Spontaneity determines whether external power is needed.

Flashcard 22: What is the unit of standard cell potential?

Answer: Volts (V). Standard unit for electrical potential difference.

Flashcard 23: What happens to the mass of the anode in a galvanic cell during operation?

Answer: It decreases. Metal atoms leave electrode as oxidation occurs.

Flashcard 24: What is the standard cell potential $(E^\theta)$ for a galvanic cell?

Answer: Positive. Spontaneous reactions have positive cell potentials.

Flashcard 25: What is the role of the salt bridge in a galvanic cell?

Answer: To maintain electrical neutrality. Allows ion migration to balance charge as reactions proceed.

Flashcard 26: What is the standard cell potential $(E^\theta)$ for an electrolytic cell?

Answer: Negative. Non-spontaneous reactions have negative cell potentials.

Flashcard 27: What is the primary function of a galvanic cell?

Answer: To convert chemical energy into electrical energy. Spontaneous redox reactions drive electron flow through external circuit.

Flashcard 28: Identify the standard conditions for measuring cell potential.

Answer: 1 M concentration, 1 atm pressure, 25°C temperature. Standard state conditions for reliable potential measurements.

Flashcard 29: What happens to the mass of the anode in a galvanic cell during operation?

Answer: It decreases. Metal atoms leave electrode as oxidation occurs.

Flashcard 30: What is the role of inert electrodes like platinum?

Answer: To conduct electrons without participating in the reaction. Provide surface for electron transfer without reacting.

Flashcard 31: What occurs at the anode in an electrolytic cell?

Answer: Oxidation. Oxidation still occurs at anode regardless of cell type.

Flashcard 32: What occurs at the cathode in an electrolytic cell?

Answer: Reduction. Reduction still occurs at cathode regardless of cell type.

Flashcard 33: What is the primary function of a galvanic cell?

Answer: To convert chemical energy into electrical energy. Spontaneous redox reactions drive electron flow through external circuit.

Flashcard 34: What is the criterion for a reaction to be spontaneous in terms of $\Delta G$?

Answer: $\Delta G < 0$. Negative free energy indicates thermodynamically favorable process.

Flashcard 35: Identify the charge of the cathode in an electrolytic cell.

Answer: Negative. Connected to negative terminal of external power source.

Flashcard 36: Calculate the equilibrium constant $K$ given $E^\theta = 0.0592$ V and $n = 1$.

Answer: $K = 10$. Using $E^\theta = \frac{0.0592}{n} \log K$ with $n=1$.

Flashcard 37: State the Nernst equation.

Answer: $E = E^\theta - \frac{RT}{nF} \ln Q$. Accounts for concentration effects on cell potential.

Flashcard 38: What is the primary function of a galvanic cell?

Answer: To convert chemical energy into electrical energy. Spontaneous redox reactions drive electron flow through external circuit.

Flashcard 39: What is the purpose of an external circuit in a galvanic cell?

Answer: To allow electron flow. Completes circuit for electron movement between electrodes.

Flashcard 40: Which metal acts as a reducing agent in a galvanic cell?

Answer: The metal at the anode. Undergoes oxidation, losing electrons to external circuit.

Flashcard 41: State the effect of temperature on cell potential.

Answer: Cell potential generally decreases with increasing temperature. Higher temperature typically reduces driving force for reaction.

Flashcard 42: State the function of a power source in an electrolytic cell.

Answer: To provide energy for non-spontaneous reactions. Overcomes negative cell potential of non-spontaneous reactions.

Flashcard 43: What happens to the mass of the anode in a galvanic cell during operation?

Answer: It decreases. Metal atoms leave electrode as oxidation occurs.

Flashcard 44: What occurs at the anode in a galvanic cell?

Answer: Oxidation. Electrons are lost, making anode the source of electrons.

Flashcard 45: What is the formula for the cell potential of a galvanic cell?

Answer: $E_{cell} = E_{cathode} - E_{anode}$. Standard reduction potential difference between electrodes.

Flashcard 46: Calculate $\Delta G$ for a cell with $n=2$, $F=96485$ C/mol, and $E_{cell}=1.1$ V.

Answer: $-212.67$ kJ/mol. Using $\Delta G = -nFE = -(2)(96485)(1.1)$.

Flashcard 47: What is the primary function of an electrolytic cell?

Answer: To convert electrical energy into chemical energy. External power source drives non-spontaneous redox reactions.

Flashcard 48: State the effect of temperature on cell potential.

Answer: Cell potential generally decreases with increasing temperature. Higher temperature typically reduces driving force for reaction.

Flashcard 49: What is the role of the salt bridge in a galvanic cell?

Answer: To maintain electrical neutrality. Allows ion migration to balance charge as reactions proceed.

Flashcard 50: What is the standard cell potential $(E^\theta)$ for a galvanic cell?

Answer: Positive. Spontaneous reactions have positive cell potentials.

Flashcard 51: State the direction of electron flow in a galvanic cell.

Answer: From anode to cathode. Electrons flow from negative anode to positive cathode.

Flashcard 52: What occurs at the cathode in a galvanic cell?

Answer: Reduction. Electrons are gained, making cathode the electron destination.

Flashcard 53: Identify the charge of the anode in a galvanic cell.

Answer: Negative. Loses electrons during oxidation, creating electron excess.

Flashcard 54: Identify the charge of the anode in a galvanic cell.

Answer: Negative. Loses electrons during oxidation, creating electron excess.

Flashcard 55: What does a negative cell potential indicate?

Answer: The reaction is non-spontaneous. External energy required to drive the reaction forward.

Flashcard 56: Which metal acts as a reducing agent in a galvanic cell?

Answer: The metal at the anode. Undergoes oxidation, losing electrons to external circuit.

Flashcard 57: What is the significance of the equilibrium constant $K$ in electrochemistry?

Answer: Relates to cell potential by $E^\theta = \frac{RT}{nF} \ln K$. Large $K$ indicates favorable reaction with positive $E^\theta$.

Flashcard 58: What occurs at the cathode in an electrolytic cell?

Answer: Reduction. Reduction still occurs at cathode regardless of cell type.