8 Questions
What is the primary function of an electrolytic cell?
To drive a chemical reaction using an external power source
Which of the following is an application of electrolytic cells?
Electroplating
What is the symbol for the electromotive force of a cell in the Nernst Equation?
E
What is the purpose of the Nernst Equation?
To predict the voltage of a cell under different conditions
What is the effect of increasing the temperature on the EMF of a cell, according to the Nernst Equation?
The EMF increases
What is the reaction quotient in the Nernst Equation?
The ratio of the concentrations of reactants to products
Which electrode is where oxidation occurs in an electrolytic cell?
Anode
What is the unit of the gas constant, R, in the Nernst Equation?
J/mol·K
Study Notes
Electrolytic Cells
- An electrolytic cell is an electrochemical cell that uses an external power source to drive a chemical reaction.
- It consists of two electrodes (an anode and a cathode) immersed in an electrolyte solution.
- The anode is the electrode where oxidation occurs, and the cathode is the electrode where reduction occurs.
- Electrolytic cells are used for various applications, including:
- Electroplating: depositing a thin layer of a metal onto the surface of another metal.
- Electrolysis: decomposition of water into hydrogen and oxygen.
- Refining of metals: purifying metals through electrolysis.
Nernst Equation
- The Nernst Equation is a mathematical formula used to determine the electromotive force (EMF) of an electrochemical cell.
- It is given by:
E = E° - (RT/nF) \* ln(Q)- E: EMF of the cell
- E°: standard EMF of the cell
- R: gas constant
- T: temperature in Kelvin
- n: number of electrons transferred
- F: Faraday's constant
- Q: reaction quotient
- The Nernst Equation relates the EMF of a cell to the standard EMF, temperature, and reaction quotient.
- It is used to calculate the EMF of a cell under non-standard conditions.
- Applications of the Nernst Equation include:
- Predicting the voltage of a cell under different conditions.
- Determining the equilibrium constant of a reaction.
- Understanding the effect of temperature and concentration on cell voltage.
Electrolytic Cells
- An electrolytic cell is a type of electrochemical cell that uses an external power source to drive a chemical reaction.
- It consists of two electrodes: an anode (where oxidation occurs) and a cathode (where reduction occurs).
- Electrolytic cells are used for various applications, including:
- Electroplating: depositing a thin layer of a metal onto the surface of another metal.
- Electrolysis: decomposing water into hydrogen and oxygen.
- Refining of metals: purifying metals through electrolysis.
Nernst Equation
- The Nernst Equation determines the electromotive force (EMF) of an electrochemical cell.
- The equation is:
E = E° - (RT/nF) * ln(Q). - Each term in the equation represents:
- E: EMF of the cell.
- E°: standard EMF of the cell.
- R: gas constant.
- T: temperature in Kelvin.
- n: number of electrons transferred.
- F: Faraday's constant.
- Q: reaction quotient.
- The Nernst Equation relates the EMF of a cell to the standard EMF, temperature, and reaction quotient.
- Applications of the Nernst Equation include:
- Predicting the voltage of a cell under different conditions.
- Determining the equilibrium constant of a reaction.
- Understanding the effect of temperature and concentration on cell voltage.
Learn about electrolytic cells, their components, and their applications in electroplating and other processes.
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