The Nernst Equation Is One Of The Most Important Equations In Electrochemistry To Calculate The Cell Potential At Non S 1 (140.61 KiB) Viewed 28 times
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 E = E° 2.303 RT Q = nFog 10Q 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, F is the Faraday constant, and Q is the reaction quotient. Using the common reference temperature, 25 °C or 298 K, the equation has the form E = E° - (0.0592) log Q The reaction quotient has the usual form [products]it [reactants] A table of standard reduction potentials gives the voltage at standard conditions, 1.00 M for all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure. Part A For the reaction 2CO³(aq) + 2C1 (aq)→2Co²(aq) + Cl2(g). E° = 0.483 V what is the cell potential at 25 °C if the concentrations are [Co³= 9.80x10-2 M, [Co² = 0.619 M, and [C1] = 0.146 M, and the pressure of C12 is PCI = 8.40 atm ? Express your answer with the appropriate units. ▸ View Available Hint(s) Templates Symbols .353 V Submit Previous Answers x Incorrect; Try Again Provide Feedback undo redo reset keyboard shortcuts help, Next >
MISSED THIS? Read Section 20.6 (Pages 917-922). A Cu/Cu²+ concentration cell has a voltage of 0.23 V at 25 °C. The concentration of Cu²+ in one of the half-cells is 1.5x10-3 M. Part A What is the concentration of Cu²+ in the other half-cell? (Assume the concentration in the unknown cell to be the lower of the two concentrations.) Express your answer using two significant figures. [Cu²+] Submit Templates Symbols 2.7.10 11 V undo redo reslet keyboard shortcuts help, Previous Answers Request Answer x Incorrect; Try Again M
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