± The Nernst Equation S 20f2 Constants 1 Pediodic Table PartA The Nemst equation
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± The Nernst Equation S 20f2 Constants 1 Pediodic Table PartA The Nemst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is For the reaction 2C03 + (aq) +2C1" (aq)?2C02+ (aq) + C13(g). E-0.483 what iste ell potential at 25-c if the concentrations are [Co3+ ]?0410 M. [Co2+] , and [Cl0.462 M, and the pressure of Cly is Pcls -9.30 atm? 0.585 M Express your answer with the appropriate units. 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. At standard temperature, 25 C or 298 K, the equation has the form View Available Hint(s) B- 0.92V The reaction quotient has the usual form Submit Previous Answers 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 Nemst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure X Incorrect; Try Again; 4 attempts remaining ( Return to Assignment Provide FeedbackExplanation / Answer
They clearly mentioned in left hand side 1.00M for all solutions and 1.00 atm for all gases.
There is no conversion between atm and Mol
Q = [cl2] [Co]^2 / [cl]^2 [co]^2
By substituting the given values we get the desired solution
0.483+0.115 = 0.598
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