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AP Chemistry Flashcards: Cell Potential Under Nonstandard Conditions

Study Cell Potential Under Nonstandard Conditions in AP Chemistry with focused flashcards that help you recognize the idea, recall the key rule, and apply it in practice-style prompts.

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What this deck covers

This deck focuses on Cell Potential Under Nonstandard Conditions, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

How to use these flashcards

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.

AP Chemistry Flashcards: Cell Potential Under Nonstandard Conditions

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QUESTION

Calculate $\Delta G$ if $n=2$ and $E=0.25\ \text{V}$ (use $F=96485\ \text{C mol}^{-1}$ ).

Tap or drag to reveal answer

ANSWER

$\Delta G=-4.82\times 10^4\ \text{J mol}^{-1}$ . $\Delta G=-(2)(96485)(0.25)=-48242.5$ J/mol.

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All flashcards

Flashcard 1: Calculate $\Delta G$ if $n=2$ and $E=0.25\ \text{V}$ (use $F=96485\ \text{C mol}^{-1}$ ).

Answer: $\Delta G=-4.82\times 10^4\ \text{J mol}^{-1}$ . $\Delta G=-(2)(96485)(0.25)=-48242.5$ J/mol.

Flashcard 2: Calculate $E^\circ$ at $25^\circ\text{C}$ if $K=1.0\times 10^6$ and $n=2$ .

Answer: $E^\circ=0.178\ \text{V}$ . $E^\circ=\frac{0.0592}{2}\log(10^6)=0.0296\times 6$ .

Flashcard 3: Calculate $K$ at $25^\circ\text{C}$ if $E^\circ=0.30\ \text{V}$ and $n=2$ .

Answer: $K=1.4\times 10^{10}$ . $0.30=\frac{0.0592}{2}\log K$ ; $\log K=10.14$ .

Flashcard 4: Find $Q$ at $25^\circ\text{C}$ if $E^\circ=0.50\ \text{V}$ , $E=0.44\ \text{V}$ , and $n=2$ .

Answer: $Q=4.0\times 10^2$ . $0.44=0.50-\frac{0.0592}{2}\log Q$ ; solve for $Q$ .

Flashcard 5: Calculate $E$ at $25^\circ\text{C}$ if $E^\circ=0.80\ \text{V}$ , $n=1$ , and $Q=10^2$ .

Answer: $E=0.68\ \text{V}$ . $E=0.80-0.0592\log(100)=0.80-0.118$ .

Flashcard 6: Calculate $E$ at $25^\circ\text{C}$ if $E^\circ=1.10\ \text{V}$ , $n=2$ , and $Q=10^{-4}$ .

Answer: $E=1.22\ \text{V}$ . $E=1.10-\frac{0.0592}{2}\log(10^{-4})=1.10+0.118$ .

Flashcard 7: What is $n$ in the Nernst equation, and how is it determined from the reaction?

Answer: $n$ is moles of electrons transferred in the balanced redox reaction. Count electrons in half-reactions after balancing.

Flashcard 8: What is the relationship between $E$ and $E^\circ$ when $Q=1$ ?

Answer: $E=E^\circ$ . Standard conditions: all activities equal 1.

Flashcard 9: What is the sign of the Nernst correction when $Q<1$ (relative to $E^\circ$ )?

Answer: $E>E^\circ$ . Reactants favored, so potential increases from standard.

Flashcard 10: What is the sign of the Nernst correction when $Q>1$ (relative to $E^\circ$ )?

Answer: $E<E^\circ$ . Products favored, so potential decreases from standard.

Flashcard 11: State the relationship between cell potential and Gibbs free energy under any conditions.

Answer: $\Delta G=-nFE$ . Negative sign shows spontaneous reactions have $E>0$ .

Flashcard 12: Identify which species are omitted from $Q$ : pure solids, pure liquids, aqueous ions, or gases.

Answer: Pure solids and pure liquids are omitted from $Q$ . Only dissolved species and gases affect cell potential.

Flashcard 13: What does $Q$ represent in the Nernst equation for an electrochemical cell?

Answer: Reaction quotient from activities in the balanced net ionic equation. Ratio of products to reactants raised to stoichiometric powers.

Flashcard 14: State the relationship between standard cell potential and standard Gibbs free energy.

Answer: $\Delta G^\circ=-nFE^\circ$ . Links thermodynamics to electrochemistry at standard state.

Flashcard 15: State the relationship between $E^\circ$ and the equilibrium constant $K$ at $25^\circ\text{C}$ .

Answer: $E^\circ=\frac{0.0592}{n}\log K$ . Derived from $\Delta G^\circ=-RT\ln K=-nFE^\circ$ .

Flashcard 16: What is the cell potential at equilibrium, and what is the corresponding value of $Q$ ?

Answer: $E=0$ and $Q=K$ . No driving force at equilibrium; $\Delta G=0$ .

Flashcard 17: Identify the direction of spontaneity when $E>0$ for the cell reaction as written.

Answer: Spontaneous as written. Positive $E$ means $\Delta G<0$ .

Flashcard 18: Identify the direction of spontaneity when $E<0$ for the cell reaction as written.

Answer: Nonspontaneous as written; spontaneous in reverse. Negative $E$ means $\Delta G>0$ forward.

Flashcard 19: State the Nernst equation at $25^\circ\text{C}$ using base-10 logarithms.

Answer: $E=E^\circ-\frac{0.0592}{n}\log Q$ . Simplified form at 298 K using $\log$ instead of $\ln$ .

Flashcard 20: State the formula for the cell potential under nonstandard conditions (Nernst equation).

Answer: $E=E^\circ-\frac{RT}{nF}\ln Q$ . Modifies standard potential by concentration effects via $\ln Q$ term.

Flashcard 21: Identify the condition on $Q$ when $E=0$ for a cell at equilibrium.

Answer: $Q=K$ . At equilibrium, $E=0$ and reaction quotient equals equilibrium constant.

Flashcard 22: State the relationship between $E^\circ$ and the equilibrium constant $K$ at $25^\circ\text{C}$ .

Answer: $E^\circ=\frac{0.0592}{n}\log K$ . Derived from $E=0$ when $Q=K$ in Nernst equation.

Flashcard 23: State the general relationship between $\Delta G$ and cell potential $E$ .

Answer: $\Delta G=-nFE$ . Relates electrical work to thermodynamic spontaneity.

Flashcard 24: State the relationship between $\Delta G^\circ$ and the equilibrium constant $K$ .

Answer: $\Delta G^\circ=-RT\ln K$ . Fundamental thermodynamic relationship at equilibrium.

Flashcard 25: Identify how $E$ changes when $Q$ increases (with $E^\circ$ , $T$ , and $n$ constant).

Answer: $E$ decreases. Larger $Q$ means more products, driving reverse reaction.

Flashcard 26: Calculate $\log K$ at $25^\circ\text{C}$ if $E^\circ=0.30\ \text{V}$ and $n=3$ .

Answer: $\log K\approx15.2$ . $0.30=\frac{0.0592}{3}\log K$ ; $\log K=\frac{0.90}{0.0592}\approx15.2$ .

Flashcard 27: State the formula for cell potential under nonstandard conditions (Nernst equation).

Answer: $E=E^\circ-\frac{RT}{nF}\ln Q$ . Modified by reaction quotient $Q$ and temperature; $n$ is electrons transferred.

Flashcard 28: State the Nernst equation at $25^\circ\text{C}$ using base-10 logarithms.

Answer: $E=E^\circ-\frac{0.0592}{n}\log Q$ . Simplified form at 298 K using $\frac{2.303RT}{F}=0.0592$ V.

Flashcard 29: What does $Q$ represent in the Nernst equation for an electrochemical cell?

Answer: Reaction quotient, products over reactants using activities. Measures reaction progress; equals $K$ at equilibrium.

Flashcard 30: What does $n$ represent in the Nernst equation for a galvanic cell?

Answer: Moles of electrons transferred in the balanced redox reaction. Count electrons in half-reaction balancing.

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AP Chemistry Flashcards: Cell Potential Under Nonstandard Conditions

Study Cell Potential Under Nonstandard Conditions in AP Chemistry with focused flashcards that help you recognize the idea, recall the key rule, and apply it in practice-style prompts.

← Back to flashcard decks

What this deck covers

This deck focuses on Cell Potential Under Nonstandard Conditions, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

How to use these flashcards

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.

AP Chemistry Flashcards: Cell Potential Under Nonstandard Conditions

/ 30

0 reviewed

0% Complete

0 reviewing

QUESTION

Calculate $\Delta G$ if $n=2$ and $E=0.25\ \text{V}$ (use $F=96485\ \text{C mol}^{-1}$ ).

Tap or drag to reveal answer

ANSWER

$\Delta G=-4.82\times 10^4\ \text{J mol}^{-1}$ . $\Delta G=-(2)(96485)(0.25)=-48242.5$ J/mol.

Swipe Right = I Know It! 🎉

Swipe Left = Still Learning

All flashcards

Flashcard 1: Calculate $\Delta G$ if $n=2$ and $E=0.25\ \text{V}$ (use $F=96485\ \text{C mol}^{-1}$ ).

Answer: $\Delta G=-4.82\times 10^4\ \text{J mol}^{-1}$ . $\Delta G=-(2)(96485)(0.25)=-48242.5$ J/mol.

Flashcard 2: Calculate $E^\circ$ at $25^\circ\text{C}$ if $K=1.0\times 10^6$ and $n=2$ .

Answer: $E^\circ=0.178\ \text{V}$ . $E^\circ=\frac{0.0592}{2}\log(10^6)=0.0296\times 6$ .

Flashcard 3: Calculate $K$ at $25^\circ\text{C}$ if $E^\circ=0.30\ \text{V}$ and $n=2$ .

Answer: $K=1.4\times 10^{10}$ . $0.30=\frac{0.0592}{2}\log K$ ; $\log K=10.14$ .

Flashcard 4: Find $Q$ at $25^\circ\text{C}$ if $E^\circ=0.50\ \text{V}$ , $E=0.44\ \text{V}$ , and $n=2$ .

Answer: $Q=4.0\times 10^2$ . $0.44=0.50-\frac{0.0592}{2}\log Q$ ; solve for $Q$ .

Flashcard 5: Calculate $E$ at $25^\circ\text{C}$ if $E^\circ=0.80\ \text{V}$ , $n=1$ , and $Q=10^2$ .

Answer: $E=0.68\ \text{V}$ . $E=0.80-0.0592\log(100)=0.80-0.118$ .

Flashcard 6: Calculate $E$ at $25^\circ\text{C}$ if $E^\circ=1.10\ \text{V}$ , $n=2$ , and $Q=10^{-4}$ .

Answer: $E=1.22\ \text{V}$ . $E=1.10-\frac{0.0592}{2}\log(10^{-4})=1.10+0.118$ .

Flashcard 7: What is $n$ in the Nernst equation, and how is it determined from the reaction?

Answer: $n$ is moles of electrons transferred in the balanced redox reaction. Count electrons in half-reactions after balancing.

Flashcard 8: What is the relationship between $E$ and $E^\circ$ when $Q=1$ ?

Answer: $E=E^\circ$ . Standard conditions: all activities equal 1.

Flashcard 9: What is the sign of the Nernst correction when $Q<1$ (relative to $E^\circ$ )?

Answer: $E>E^\circ$ . Reactants favored, so potential increases from standard.

Flashcard 10: What is the sign of the Nernst correction when $Q>1$ (relative to $E^\circ$ )?

Answer: $E<E^\circ$ . Products favored, so potential decreases from standard.

Flashcard 11: State the relationship between cell potential and Gibbs free energy under any conditions.

Answer: $\Delta G=-nFE$ . Negative sign shows spontaneous reactions have $E>0$ .

Flashcard 12: Identify which species are omitted from $Q$ : pure solids, pure liquids, aqueous ions, or gases.

Answer: Pure solids and pure liquids are omitted from $Q$ . Only dissolved species and gases affect cell potential.

Flashcard 13: What does $Q$ represent in the Nernst equation for an electrochemical cell?

Answer: Reaction quotient from activities in the balanced net ionic equation. Ratio of products to reactants raised to stoichiometric powers.

Flashcard 14: State the relationship between standard cell potential and standard Gibbs free energy.

Answer: $\Delta G^\circ=-nFE^\circ$ . Links thermodynamics to electrochemistry at standard state.

Flashcard 15: State the relationship between $E^\circ$ and the equilibrium constant $K$ at $25^\circ\text{C}$ .

Answer: $E^\circ=\frac{0.0592}{n}\log K$ . Derived from $\Delta G^\circ=-RT\ln K=-nFE^\circ$ .

Flashcard 16: What is the cell potential at equilibrium, and what is the corresponding value of $Q$ ?

Answer: $E=0$ and $Q=K$ . No driving force at equilibrium; $\Delta G=0$ .

Flashcard 17: Identify the direction of spontaneity when $E>0$ for the cell reaction as written.

Answer: Spontaneous as written. Positive $E$ means $\Delta G<0$ .

Flashcard 18: Identify the direction of spontaneity when $E<0$ for the cell reaction as written.

Answer: Nonspontaneous as written; spontaneous in reverse. Negative $E$ means $\Delta G>0$ forward.

Flashcard 19: State the Nernst equation at $25^\circ\text{C}$ using base-10 logarithms.

Answer: $E=E^\circ-\frac{0.0592}{n}\log Q$ . Simplified form at 298 K using $\log$ instead of $\ln$ .

Flashcard 20: State the formula for the cell potential under nonstandard conditions (Nernst equation).

Answer: $E=E^\circ-\frac{RT}{nF}\ln Q$ . Modifies standard potential by concentration effects via $\ln Q$ term.

Flashcard 21: Identify the condition on $Q$ when $E=0$ for a cell at equilibrium.

Answer: $Q=K$ . At equilibrium, $E=0$ and reaction quotient equals equilibrium constant.

Flashcard 22: State the relationship between $E^\circ$ and the equilibrium constant $K$ at $25^\circ\text{C}$ .

Answer: $E^\circ=\frac{0.0592}{n}\log K$ . Derived from $E=0$ when $Q=K$ in Nernst equation.

Flashcard 23: State the general relationship between $\Delta G$ and cell potential $E$ .

Answer: $\Delta G=-nFE$ . Relates electrical work to thermodynamic spontaneity.

Flashcard 24: State the relationship between $\Delta G^\circ$ and the equilibrium constant $K$ .

Answer: $\Delta G^\circ=-RT\ln K$ . Fundamental thermodynamic relationship at equilibrium.

Flashcard 25: Identify how $E$ changes when $Q$ increases (with $E^\circ$ , $T$ , and $n$ constant).

Answer: $E$ decreases. Larger $Q$ means more products, driving reverse reaction.

Flashcard 26: Calculate $\log K$ at $25^\circ\text{C}$ if $E^\circ=0.30\ \text{V}$ and $n=3$ .

Answer: $\log K\approx15.2$ . $0.30=\frac{0.0592}{3}\log K$ ; $\log K=\frac{0.90}{0.0592}\approx15.2$ .

Flashcard 27: State the formula for cell potential under nonstandard conditions (Nernst equation).

Answer: $E=E^\circ-\frac{RT}{nF}\ln Q$ . Modified by reaction quotient $Q$ and temperature; $n$ is electrons transferred.

Flashcard 28: State the Nernst equation at $25^\circ\text{C}$ using base-10 logarithms.

Answer: $E=E^\circ-\frac{0.0592}{n}\log Q$ . Simplified form at 298 K using $\frac{2.303RT}{F}=0.0592$ V.

Flashcard 29: What does $Q$ represent in the Nernst equation for an electrochemical cell?

Answer: Reaction quotient, products over reactants using activities. Measures reaction progress; equals $K$ at equilibrium.

Flashcard 30: What does $n$ represent in the Nernst equation for a galvanic cell?

Answer: Moles of electrons transferred in the balanced redox reaction. Count electrons in half-reaction balancing.

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AP Chemistry Flashcards: Cell Potential Under Nonstandard Conditions

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AP Chemistry Flashcards: Cell Potential Under Nonstandard Conditions

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Flashcard 1: Calculate ΔG\Delta GΔG if n=2n=2n=2 and E=0.25 VE=0.25\ \text{V}E=0.25 V (use F=96485 C mol−1F=96485\ \text{C mol}^{-1}F=96485 C mol−1).

Flashcard 2: Calculate E∘E^\circE∘ at 25∘C25^\circ\text{C}25∘C if K=1.0×106K=1.0\times 10^6K=1.0×106 and n=2n=2n=2.

Flashcard 3: Calculate KKK at 25∘C25^\circ\text{C}25∘C if E∘=0.30 VE^\circ=0.30\ \text{V}E∘=0.30 V and n=2n=2n=2.

Flashcard 4: Find QQQ at 25∘C25^\circ\text{C}25∘C if E∘=0.50 VE^\circ=0.50\ \text{V}E∘=0.50 V, E=0.44 VE=0.44\ \text{V}E=0.44 V, and n=2n=2n=2.

Flashcard 5: Calculate EEE at 25∘C25^\circ\text{C}25∘C if E∘=0.80 VE^\circ=0.80\ \text{V}E∘=0.80 V, n=1n=1n=1, and Q=102Q=10^2Q=102.

Flashcard 6: Calculate EEE at 25∘C25^\circ\text{C}25∘C if E∘=1.10 VE^\circ=1.10\ \text{V}E∘=1.10 V, n=2n=2n=2, and Q=10−4Q=10^{-4}Q=10−4.

Flashcard 7: What is nnn in the Nernst equation, and how is it determined from the reaction?

Flashcard 8: What is the relationship between EEE and E∘E^\circE∘ when Q=1Q=1Q=1?

Flashcard 9: What is the sign of the Nernst correction when Q<1Q<1Q<1 (relative to E∘E^\circE∘)?

Flashcard 10: What is the sign of the Nernst correction when Q>1Q>1Q>1 (relative to E∘E^\circE∘)?

Flashcard 11: State the relationship between cell potential and Gibbs free energy under any conditions.

Flashcard 12: Identify which species are omitted from QQQ: pure solids, pure liquids, aqueous ions, or gases.

Flashcard 13: What does QQQ represent in the Nernst equation for an electrochemical cell?

Flashcard 14: State the relationship between standard cell potential and standard Gibbs free energy.

Flashcard 15: State the relationship between E∘E^\circE∘ and the equilibrium constant KKK at 25∘C25^\circ\text{C}25∘C.

Flashcard 16: What is the cell potential at equilibrium, and what is the corresponding value of QQQ?

Flashcard 17: Identify the direction of spontaneity when E>0E>0E>0 for the cell reaction as written.

Flashcard 18: Identify the direction of spontaneity when E<0E<0E<0 for the cell reaction as written.

Flashcard 19: State the Nernst equation at 25∘C25^\circ\text{C}25∘C using base-10 logarithms.

Flashcard 20: State the formula for the cell potential under nonstandard conditions (Nernst equation).

Flashcard 21: Identify the condition on QQQ when E=0E=0E=0 for a cell at equilibrium.

Flashcard 22: State the relationship between E∘E^\circE∘ and the equilibrium constant KKK at 25∘C25^\circ\text{C}25∘C.

Flashcard 23: State the general relationship between ΔG\Delta GΔG and cell potential EEE.

Flashcard 24: State the relationship between ΔG∘\Delta G^\circΔG∘ and the equilibrium constant KKK.

Flashcard 25: Identify how EEE changes when QQQ increases (with E∘E^\circE∘, TTT, and nnn constant).

Flashcard 26: Calculate log⁡K\log KlogK at 25∘C25^\circ\text{C}25∘C if E∘=0.30 VE^\circ=0.30\ \text{V}E∘=0.30 V and n=3n=3n=3.

Flashcard 27: State the formula for cell potential under nonstandard conditions (Nernst equation).

Flashcard 28: State the Nernst equation at 25∘C25^\circ\text{C}25∘C using base-10 logarithms.

Flashcard 29: What does QQQ represent in the Nernst equation for an electrochemical cell?

Flashcard 30: What does nnn represent in the Nernst equation for a galvanic cell?

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AP Chemistry Flashcards: Cell Potential Under Nonstandard Conditions

What this deck covers

How to use these flashcards

AP Chemistry Flashcards: Cell Potential Under Nonstandard Conditions

All flashcards

Flashcard 1: Calculate ΔG\Delta GΔG if n=2n=2n=2 and E=0.25 VE=0.25\ \text{V}E=0.25 V (use F=96485 C mol−1F=96485\ \text{C mol}^{-1}F=96485 C mol−1).

Flashcard 2: Calculate E∘E^\circE∘ at 25∘C25^\circ\text{C}25∘C if K=1.0×106K=1.0\times 10^6K=1.0×106 and n=2n=2n=2.

Flashcard 3: Calculate KKK at 25∘C25^\circ\text{C}25∘C if E∘=0.30 VE^\circ=0.30\ \text{V}E∘=0.30 V and n=2n=2n=2.

Flashcard 4: Find QQQ at 25∘C25^\circ\text{C}25∘C if E∘=0.50 VE^\circ=0.50\ \text{V}E∘=0.50 V, E=0.44 VE=0.44\ \text{V}E=0.44 V, and n=2n=2n=2.

Flashcard 5: Calculate EEE at 25∘C25^\circ\text{C}25∘C if E∘=0.80 VE^\circ=0.80\ \text{V}E∘=0.80 V, n=1n=1n=1, and Q=102Q=10^2Q=102.

Flashcard 6: Calculate EEE at 25∘C25^\circ\text{C}25∘C if E∘=1.10 VE^\circ=1.10\ \text{V}E∘=1.10 V, n=2n=2n=2, and Q=10−4Q=10^{-4}Q=10−4.

Flashcard 7: What is nnn in the Nernst equation, and how is it determined from the reaction?

Flashcard 8: What is the relationship between EEE and E∘E^\circE∘ when Q=1Q=1Q=1?

Flashcard 9: What is the sign of the Nernst correction when Q<1Q<1Q<1 (relative to E∘E^\circE∘)?

Flashcard 10: What is the sign of the Nernst correction when Q>1Q>1Q>1 (relative to E∘E^\circE∘)?

Flashcard 11: State the relationship between cell potential and Gibbs free energy under any conditions.

Flashcard 12: Identify which species are omitted from QQQ: pure solids, pure liquids, aqueous ions, or gases.

Flashcard 13: What does QQQ represent in the Nernst equation for an electrochemical cell?

Flashcard 14: State the relationship between standard cell potential and standard Gibbs free energy.

Flashcard 15: State the relationship between E∘E^\circE∘ and the equilibrium constant KKK at 25∘C25^\circ\text{C}25∘C.

Flashcard 16: What is the cell potential at equilibrium, and what is the corresponding value of QQQ?

Flashcard 17: Identify the direction of spontaneity when E>0E>0E>0 for the cell reaction as written.

Flashcard 18: Identify the direction of spontaneity when E<0E<0E<0 for the cell reaction as written.

Flashcard 19: State the Nernst equation at 25∘C25^\circ\text{C}25∘C using base-10 logarithms.

Flashcard 20: State the formula for the cell potential under nonstandard conditions (Nernst equation).

Flashcard 21: Identify the condition on QQQ when E=0E=0E=0 for a cell at equilibrium.

Flashcard 22: State the relationship between E∘E^\circE∘ and the equilibrium constant KKK at 25∘C25^\circ\text{C}25∘C.

Flashcard 23: State the general relationship between ΔG\Delta GΔG and cell potential EEE.

Flashcard 24: State the relationship between ΔG∘\Delta G^\circΔG∘ and the equilibrium constant KKK.

Flashcard 25: Identify how EEE changes when QQQ increases (with E∘E^\circE∘, TTT, and nnn constant).

Flashcard 26: Calculate log⁡K\log KlogK at 25∘C25^\circ\text{C}25∘C if E∘=0.30 VE^\circ=0.30\ \text{V}E∘=0.30 V and n=3n=3n=3.

Flashcard 27: State the formula for cell potential under nonstandard conditions (Nernst equation).

Flashcard 28: State the Nernst equation at 25∘C25^\circ\text{C}25∘C using base-10 logarithms.

Flashcard 29: What does QQQ represent in the Nernst equation for an electrochemical cell?

Flashcard 30: What does nnn represent in the Nernst equation for a galvanic cell?

Flashcard 1: Calculate $\Delta G$ if $n=2$ and $E=0.25\ \text{V}$ (use $F=96485\ \text{C mol}^{-1}$ ).

Flashcard 2: Calculate $E^\circ$ at $25^\circ\text{C}$ if $K=1.0\times 10^6$ and $n=2$ .

Flashcard 3: Calculate $K$ at $25^\circ\text{C}$ if $E^\circ=0.30\ \text{V}$ and $n=2$ .

Flashcard 4: Find $Q$ at $25^\circ\text{C}$ if $E^\circ=0.50\ \text{V}$ , $E=0.44\ \text{V}$ , and $n=2$ .

Flashcard 5: Calculate $E$ at $25^\circ\text{C}$ if $E^\circ=0.80\ \text{V}$ , $n=1$ , and $Q=10^2$ .

Flashcard 6: Calculate $E$ at $25^\circ\text{C}$ if $E^\circ=1.10\ \text{V}$ , $n=2$ , and $Q=10^{-4}$ .

Flashcard 7: What is $n$ in the Nernst equation, and how is it determined from the reaction?

Flashcard 8: What is the relationship between $E$ and $E^\circ$ when $Q=1$ ?

Flashcard 9: What is the sign of the Nernst correction when $Q<1$ (relative to $E^\circ$ )?

Flashcard 10: What is the sign of the Nernst correction when $Q>1$ (relative to $E^\circ$ )?

Flashcard 12: Identify which species are omitted from $Q$ : pure solids, pure liquids, aqueous ions, or gases.

Flashcard 13: What does $Q$ represent in the Nernst equation for an electrochemical cell?

Flashcard 15: State the relationship between $E^\circ$ and the equilibrium constant $K$ at $25^\circ\text{C}$ .

Flashcard 16: What is the cell potential at equilibrium, and what is the corresponding value of $Q$ ?

Flashcard 17: Identify the direction of spontaneity when $E>0$ for the cell reaction as written.

Flashcard 18: Identify the direction of spontaneity when $E<0$ for the cell reaction as written.

Flashcard 19: State the Nernst equation at $25^\circ\text{C}$ using base-10 logarithms.

Flashcard 21: Identify the condition on $Q$ when $E=0$ for a cell at equilibrium.

Flashcard 22: State the relationship between $E^\circ$ and the equilibrium constant $K$ at $25^\circ\text{C}$ .

Flashcard 23: State the general relationship between $\Delta G$ and cell potential $E$ .

Flashcard 24: State the relationship between $\Delta G^\circ$ and the equilibrium constant $K$ .

Flashcard 25: Identify how $E$ changes when $Q$ increases (with $E^\circ$ , $T$ , and $n$ constant).

Flashcard 26: Calculate $\log K$ at $25^\circ\text{C}$ if $E^\circ=0.30\ \text{V}$ and $n=3$ .

Flashcard 28: State the Nernst equation at $25^\circ\text{C}$ using base-10 logarithms.

Flashcard 29: What does $Q$ represent in the Nernst equation for an electrochemical cell?

Flashcard 30: What does $n$ represent in the Nernst equation for a galvanic cell?

Flashcard 1: Calculate $\Delta G$ if $n=2$ and $E=0.25\ \text{V}$ (use $F=96485\ \text{C mol}^{-1}$ ).

Flashcard 2: Calculate $E^\circ$ at $25^\circ\text{C}$ if $K=1.0\times 10^6$ and $n=2$ .

Flashcard 3: Calculate $K$ at $25^\circ\text{C}$ if $E^\circ=0.30\ \text{V}$ and $n=2$ .

Flashcard 4: Find $Q$ at $25^\circ\text{C}$ if $E^\circ=0.50\ \text{V}$ , $E=0.44\ \text{V}$ , and $n=2$ .

Flashcard 5: Calculate $E$ at $25^\circ\text{C}$ if $E^\circ=0.80\ \text{V}$ , $n=1$ , and $Q=10^2$ .

Flashcard 6: Calculate $E$ at $25^\circ\text{C}$ if $E^\circ=1.10\ \text{V}$ , $n=2$ , and $Q=10^{-4}$ .

Flashcard 7: What is $n$ in the Nernst equation, and how is it determined from the reaction?

Flashcard 8: What is the relationship between $E$ and $E^\circ$ when $Q=1$ ?

Flashcard 9: What is the sign of the Nernst correction when $Q<1$ (relative to $E^\circ$ )?

Flashcard 10: What is the sign of the Nernst correction when $Q>1$ (relative to $E^\circ$ )?

Flashcard 12: Identify which species are omitted from $Q$ : pure solids, pure liquids, aqueous ions, or gases.

Flashcard 13: What does $Q$ represent in the Nernst equation for an electrochemical cell?

Flashcard 15: State the relationship between $E^\circ$ and the equilibrium constant $K$ at $25^\circ\text{C}$ .

Flashcard 16: What is the cell potential at equilibrium, and what is the corresponding value of $Q$ ?

Flashcard 17: Identify the direction of spontaneity when $E>0$ for the cell reaction as written.

Flashcard 18: Identify the direction of spontaneity when $E<0$ for the cell reaction as written.

Flashcard 19: State the Nernst equation at $25^\circ\text{C}$ using base-10 logarithms.

Flashcard 21: Identify the condition on $Q$ when $E=0$ for a cell at equilibrium.

Flashcard 22: State the relationship between $E^\circ$ and the equilibrium constant $K$ at $25^\circ\text{C}$ .

Flashcard 23: State the general relationship between $\Delta G$ and cell potential $E$ .

Flashcard 24: State the relationship between $\Delta G^\circ$ and the equilibrium constant $K$ .

Flashcard 25: Identify how $E$ changes when $Q$ increases (with $E^\circ$ , $T$ , and $n$ constant).

Flashcard 26: Calculate $\log K$ at $25^\circ\text{C}$ if $E^\circ=0.30\ \text{V}$ and $n=3$ .

Flashcard 28: State the Nernst equation at $25^\circ\text{C}$ using base-10 logarithms.

Flashcard 29: What does $Q$ represent in the Nernst equation for an electrochemical cell?

Flashcard 30: What does $n$ represent in the Nernst equation for a galvanic cell?