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physicsperson
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For an electrochemical cell containing two metals how do I figure out which one reduces and which one oxidizes using standard reduction potentials? Thank you very much for the help.
physicsperson said:For an electrochemical cell containing two metals how do I figure out which one reduces and which one oxidizes using standard reduction potentials? Thank you very much for the help.
The reducing agent in an electrochemical cell is the metal that undergoes oxidation, meaning it loses electrons. To determine which metal is the reducing agent, you can observe the direction of electron flow in the cell. The metal at the anode, where oxidation occurs, is the reducing agent.
Yes, a voltmeter can be used to determine which metal is the reducing agent in an electrochemical cell. By measuring the potential difference between the two electrodes, you can determine which metal has a higher tendency to lose electrons and is therefore the reducing agent.
The standard reduction potential is a measure of a metal's tendency to gain electrons. The metal with a more negative standard reduction potential will be the reducing agent in the electrochemical cell, as it has a greater tendency to lose electrons and undergo oxidation.
The electrolyte solution in an electrochemical cell provides the medium for ions to flow between the two electrodes. It also affects the reduction potential of the metals by providing a source of ions for the reduction reactions to occur. The type and concentration of the electrolyte can impact which metal is the reducing agent.
Yes, the activity series is a list of metals in order of their reactivity. The metal at the top of the activity series will be the reducing agent in an electrochemical cell, as it has the highest tendency to lose electrons. However, this is only applicable for single replacement reactions and not for all electrochemical cells.