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| What does a half-cell contain? |
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Definition
Either... An element electrode in contact with its aqueous ions Or... Two different aqueous ions of the same element in different oxidation states using platimum as the electrode. |
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Term
Define the standard electrode potential of a half-cell (Eθ). |
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Definition
| The standard electrode potential of a half-cell is the voltage of a half-cell compared with a standard hydrogen electrode. |
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Term
| What is the standard electrode potential of a half-cell a measure of? What are it units? |
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Definition
| The standard electrode potential of a half-cell is a measure of the ease with which one oxidation state in a half-cell can be converted into another oxidation state. Standard electrode potential is measured in volts. |
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Term
| What conditions are necessary when measuring an Eθ value? |
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Definition
Standard conditions are necessary when measuring an Eθ value. Standard conditions are: |
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Term
Q1) What do two half-cells put together form? Q2) How can the cell voltage be calculated? |
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Definition
A1) Two half-cells put together form an electrochemical cell. A2) The cell voltage of an elctrochemical cell can be calculated by finding the difference between the standard electrode potentials of the 2 half cells OR Mrs Wheeler's way: Line up the half equations the "right way", changing the Eθ values sign accordingly. Then add the two Eθ values together to obtain ΔEθ. |
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Term
| For a particular redox reaction to occur, must the standard electrode potential of the half-equation involving the species being reduced be more or less positive than the standard electrode potential of the half-equation involving the species being oxidised? |
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Definition
| For a particular redox reaction to occur, the standard elctrode potential of the half-equation involving the species being reduced (oxidising agent) must be more positive than the standard electrode potential of the half-equation involving the species being oxidised. |
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