The Nemst equation is one of the most important equations in electrochemistry. T

Question

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 E=E degree -2.303RT/nF Log10Q where E is the potential in volts. En 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 degrees C or 298 K. the equation has the form E=E degree -(0.0592/n) log Q The reaction quotient has the usual form Q= [products]z/ [reactants]v A table of standard reduction potentials gives the voltage at standard conditions. 100 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. For the reaction 2Co3+ (aq) + 2Cl (aq) rightarrow 2CO2+ (aq) + Cl2(g). E = 0.71 V what is the cell potential at 25 degrees C if the concentrations are [CO3+] = 0.102M. [CO2+ ] = 0.756M. and [Cl ] = 0.640Mand the pressure of CI2 is Pcl2 = 7.30atm ?

Explanation / Answer

We will need to use

E = E

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