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Questions and Answers
What is an electrochemical cell?
What is an electrochemical cell?
A device that converts chemical energy into electrical energy and vice versa. It consists of two electrodes immersed in one or more suitable electrolytes.
Where does oxidation take place in an electrochemical cell?
Where does oxidation take place in an electrochemical cell?
What is the role of electrolytes in an electrochemical cell?
What is the role of electrolytes in an electrochemical cell?
Electrolytes are the medium that facilitates the flow of ions between electrodes.
How are oxidation and reduction reactions separated in a galvanic cell?
How are oxidation and reduction reactions separated in a galvanic cell?
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A galvanic cell produces electricity as a result of chemical reactions that are non-spontaneous.
A galvanic cell produces electricity as a result of chemical reactions that are non-spontaneous.
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An electrolytic cell uses electrical energy to drive a chemical reaction.
An electrolytic cell uses electrical energy to drive a chemical reaction.
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The anode is the ______ terminal in a galvanic cell.
The anode is the ______ terminal in a galvanic cell.
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What is the purpose of a salt bridge in a galvanic cell?
What is the purpose of a salt bridge in a galvanic cell?
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Explain the difference between the flow of electrons and the flow of electric current in a galvanic cell.
Explain the difference between the flow of electrons and the flow of electric current in a galvanic cell.
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What is the purpose of the vertical line or semicolon in the representation of an electrochemical cell?
What is the purpose of the vertical line or semicolon in the representation of an electrochemical cell?
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What does the double line (//) indicate in the representation of an electrochemical cell?
What does the double line (//) indicate in the representation of an electrochemical cell?
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Which of the following factors affect the electrode potential of a cell?
Which of the following factors affect the electrode potential of a cell?
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What is the EMF or cell potential of a cell?
What is the EMF or cell potential of a cell?
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How is EMF expressed?
How is EMF expressed?
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What is the formula for calculating the EMF of a cell?
What is the formula for calculating the EMF of a cell?
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What is the electrochemical series, and what is another name for it?
What is the electrochemical series, and what is another name for it?
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Which of the following factors is not a major application of the electrochemical series?
Which of the following factors is not a major application of the electrochemical series?
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What does the standard electrode potential refer to?
What does the standard electrode potential refer to?
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What is the Nernst equation, and what is its role in electrochemistry?
What is the Nernst equation, and what is its role in electrochemistry?
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What is the equilibrium constant for a cell reaction?
What is the equilibrium constant for a cell reaction?
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How does the Nernst equation relate the standard cell potential and the equilibrium constant?
How does the Nernst equation relate the standard cell potential and the equilibrium constant?
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The concentration of ions in a solution does not affect the electrode potential.
The concentration of ions in a solution does not affect the electrode potential.
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What is the primary application of the Nernst equation in electrochemistry?
What is the primary application of the Nernst equation in electrochemistry?
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At equilibrium, the change in Gibbs free energy for a cell reaction is zero.
At equilibrium, the change in Gibbs free energy for a cell reaction is zero.
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Study Notes
Electrochemical Cells
- Electrochemical cells convert chemical energy to electrical energy, or vice versa.
- They consist of two electrodes immersed in electrolytes.
Electrodes and Electrolytes
- Anode: Where oxidation occurs.
- Cathode: Where reduction occurs.
- Electrolytes: Conduct ions between electrodes.
Oxidation and Reduction Reactions
- Oxidation and reduction reactions often occur in separate containers, not physically touching.
Galvanic vs. Electrolytic Cells
- Galvanic cells: Produce electricity due to spontaneous reactions.
- Electrolytic cells: Need external energy to drive non-spontaneous reactions.
Simple Galvanic Cell (Daniel Cell)
- Contains a zinc rod in ZnSO₄ solution and a copper rod in CuSO₄ solution.
- A salt bridge completes the circuit and prevents mixing.
Reactions at the Anode
- Oxidation occurs at the anode.
- Example: Zn(s) → Zn²⁺(aq) + 2e⁻
Reactions at the Cathode
- Reduction occurs at the cathode.
- Example: Cu²⁺(aq) + 2e⁻ → Cu(s)
Electron Flow in a Galvanic Cell
- Electrons flow from the anode to the cathode.
- Electric current flows in the opposite direction.
Functions of Salt Bridge
- Completes the circuit.
- Permits ion flow between half-cells.
- Prevents intermixing of solutions.
- Prevents liquid junction potential.
Representation of an Electrochemical Cell
- Anode is always on the left, cathode on the right.
- Metal/cation, then electrolyte/cation, separated by a single bar (/) or semicolon (;).
- Salt bridge is shown by two bars (//).
Electrode Potential and EMF
- Electrode potential depends on metal type, ion concentration, and temperature.
- EMF is the difference in electrode potential.
- EMF = Ecathode - Eanode. This equation shows difference in potential is important to calculate the total.
Electrochemical Series
- Arranges elements based on increasing reduction potential.
- Also known as activity series.
- This series is helpful in predicting feasibility of reactions and relative strengths of oxidizing and reducing agents
Example Calculations (Nernst Equation)
- Calculating cell potential using Nernst equation involving various electrode potentials and concentrations at specific temperature.
Calculation of Equilibrium Constant
- Calculate equilibrium constant using cell potential and number of electrons involved in the reaction.
- Equilibrium constant shows the ratio of products to reactants at equilibrium.
Determining Ion Concentration
- Determine concentration of one ion when other ion concentration is known in a cell using the Nernst equation.
Determining pH Calculation
- Calculate pH of a solution given the relevant electrochemical data, for example half cell potentials under given conditions.
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Description
This quiz covers the fundamental concepts of electrochemical cells, including their components, types, and the reactions occurring at the electrodes. Learn about galvanic and electrolytic cells, as well as specific examples like the Daniel Cell. Test your understanding of oxidation and reduction reactions in electrochemistry.
