Term
| For any two metals in an activity series, which metal is more readily oxidized? |
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Definition
| for any two metals in an activity series, the more active metal is the more readily oxidized. |
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Term
| What type of chemical reaction is involved in all electrochemical processes? |
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Definition
| all electrochemical processes involve redox reactions. |
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Term
| How does a voltaic cell produce electrical energy? |
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Definition
| electrical energy is produced in a voltaic cell by spontaneous redox reactions within the cell. |
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Term
| What current technologies use electrochemical processes to produce electrical energy? |
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Definition
| current technologies that use electrochemical processes to produce electrical energy include dry cells, lead storage batteries, and fuel cells. |
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Term
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Definition
| any coversion between chemical energy and electrical energy. |
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Term
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Definition
| any device that converts chemical energy into electrical energy or electrical energy into chemical energy. |
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Term
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Definition
| electrochemical cells used to convert chemical energy into electrical energy. |
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Term
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Definition
| one part of a voltaic cell in which either oxidation or reduction occurs. |
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Term
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Definition
| a tube containing a strong electrolyte, often potassuim sulfate (K2SO4), connecting the two half-cells. |
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Term
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Definition
| a conductor in a circuit that carries electrons to or from a substance other than a metal. |
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Term
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Definition
| the electrode at which oxidation occurs. |
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Term
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Definition
| the electrode at which reduction occurs. |
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Term
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Definition
| a voltaic cell in which the electrolyte is a paste. |
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Term
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Definition
| a group of cells connected together. |
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Term
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Definition
| voltaic cells in which a fuel substance undergoes oxidation and from which electrical energy is continuously obtained. |
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Term
| What causes the electrical potential of an electrochemical cell? |
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Definition
| the electric potential of a cell results from a competition for electrons between two half-cells. |
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Term
| What value is assigned to the electrical potential of a standard hydrogen electrode? |
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Definition
| the standard reduction potential of the hydrogen electrode has been assigned a value of 0.00 V. |
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Term
| How can you determine the standard reduction potential of a half-cell? |
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Definition
| you can determine the standard reduction potential of a half-cell by using a standard hydrogen electrode and the equation for standard cell potential. |
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Term
| How can you interpret the cell potential of a redox reaction in terms of the spontaneity of the reaction? |
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Definition
| if the cell potential for a given redox reaction is positive, then the reaction is spontaneous as written. If the cell potential is negative, then the reaction is nonspontaneous. |
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Term
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Definition
| a measure of the voltaic cell's ability to produce an electric current. |
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Term
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Definition
| the tendency of a given half-reaction to occur as a reduction. |
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Term
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Definition
| the difference between the reduction potentials of the two half-cells. |
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Term
| Standard cell potential (E^0cell) |
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Definition
| the measured cell potential when the ion concentrations in the half-cells are 1M, any gases are at a pressure of 101 kPa, and the temperature is 25 degrees C. |
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Term
| Standard hydrogen electrode |
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Definition
| used with other electrodes so the reduction potentials of the other cells can be measured. |
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Term
| How do voltaic and electrolytic cells differ? |
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Definition
| the key difference between voltaic and electrolytic cells is that in a voltaic cell, the flow of electrons is the result of a spontaneous redox reaction, whereas in an electrolytic cell, electrons are pushed by an outside power source, such as a battery. |
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Term
| What products are formed by the electrolysis of water? |
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Definition
| the products of the electrolysis of water are hydrogen gas and oxygen gas. |
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Term
| What oxidation and reduction reactions occur during the electrolysis of brine? |
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Definition
| during electrolysis of brine, chloride ions are oxidized to produce chlorine gas at the anode. Water is reduced to produce hydrogen gas at the cathode. |
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Term
| How are electrolytic cells used in metal processing? |
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Definition
| electrolytic cells are commonly used in the plating, purifying, and refining of metals. |
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Term
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Definition
| the process in which electrical energy is used to bring about such a chemical change. |
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Term
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Definition
| an electrochemical cell used to cause a chemical change through the application of electrical energy. |
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