Question:

The Nernst equation is one of the most important equations

The Nernst equation is one of the most important equations

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/nF) * log10 where E is the potential in volts, Eº 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, and F is the Faraday constant, and is the reaction quotient. Using the common reference temperature, 25 °C or 298 K, the equation has the form E = E˚-[(0.0592)/n] log Q The reaction quotient has the usual form Q =[products]"/[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. For the reaction 2Co³+ (aq) + 2Cl-(aq)→2Co²+ (aq) + Cl₂ (g). Eº = 0.483 V what is the cell potential at 25°C if the concentrations are [Co³+] =0.598M, [Co²+]= 0.773M and [Cl-]= 0.890M and the pressure of Cl₂ is PCl2 = 5.30 atm ? Express your answer with the appropriate units.

Show Answer

Create an account. Get free access to expert answers

  • Get 3 free question credits
  • Claim your daily rewards
  • Ask your questions by snapping

Already have an account? Login