In a galvanic cell, 2 moles of electrons flow through the circuit during a reaction. Calculate the cell's standard cell potential (E°) if the reactants and products are at standard conditions.
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To calculate the standard cell potential (E°), we need to use the equation:
E° = (E°cathode) - (E°anode)
However, since we don't have any information about specific electrodes, we can use the Nernst equation:
E = E° - (RT/nF)ln(Q)
Where:
- E is the cell potential under nonstandard conditions
- R is the ideal gas constant (8.314 J/mol·K)
- T is the temperature in Kelvin
- n is the number of moles of electrons transferred in the balanced equation
- F is the Faraday constant (96,485 C/mol)
- Q is the reaction quotient, which can be calculated using the concentrations of the reactants and products
In this case, since the reactants and products are at standard conditions, the standard cell potential (E°) can be calculated by using the Nernst equation as follows:
E° = E + (RT/nF)ln(Q)
Since the reaction involves the transfer of 2 moles of electrons, n = 2.
However, we don't have specific values for E, T, or Q, so we cannot calculate the exact value for E°.
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