$$ E_{\text {cell }}=E_{c \text { cell }}^{o}-\left(\frac{R T}{n F}\right) \ln Q $$
Homework Answers
If you would have provided the choices too, answers would have been more accurate! To match with the given options/choices.
1. Ecell= potential of cell
2. E°cell = standard potential of cell (standard reduction potential of cell)
3. R = universal gas constant (8.314 J/mol kelvin)
4. T= temperature in kelvin (absolute temperature, generally 298°C)
5. n= no. of electrons(in oxidation half / reduction half reactions) or at anode or cathode
6. F= faraday constant (96500 cb/mol) or 96494
7. Q = reaction quotient (ratio of concentrations of anode, cathode OR oxidised to reduced ions)
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Electrochemical cell potential can be calculated using the Nernst equation.
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The cell potential of a redox reaction occurring in an
electrochemical cell under any set of temperature and concentration
conditions can be determined from the standard cell potential of
the cell using the Nernst equation where E is the cell
potential of the cell, E° is the standard cell potential
of the cell, R is the gas constant, T is the
temperature in kelvin, n is the moles of electrons
transferred in the reaction, and Q is the reaction
quotient....
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The cell potential of a redox reaction occurring in an
electrochemical cell under any set of temperature and concentration
conditions can be determined from the standard cell potential of
the cell using the Nernst equation where E is the cell
potential of the cell, E° is the standard cell potential
of the cell, R is the gas constant, T is the
temperature in kelvin, n is the moles of electrons
transferred in the reaction, and Q is the reaction
quotient....
Using the electrochemical series and the standard reduction potential tables in your text, would you be able to form a galvanic cell using chromium and silver? If so, what would be the Ecell for the galvanic cell, what would be the overall bal anced equation, and what would be the electrolyte solutions for each half cell? (2 points total)
+ The Nernst Equation 4 of 5 A Review Constants Periodic Ta The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is Part A EN E 2.303 RT 10g10 Q For the reaction where E is the potential in volts, E is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred,...
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