Calculating Energy in Electrochemical Processes

Key Questions

• What is the Nernst equation?

  The Nernst equation is an equation that relates the reduction potential of a half-cell at any point in time to the standard electrode potential, temperature, activity, and reaction quotient of the underlying reactions and species used.

  It is named after the German physical chemist who first formulated it, Walther Nernst.

  

  Deevona · · Jul 29 2014
• Why is the Nernst equation important?

  The Nernst equation #E^0=E^theta+(RT)/(nF)ln("Oxidants"/"Reductant")#

  It has other forms; but basically, it shows us the relationship between Electrode potential of a half cell and Temperature.

  It is a direct relationship. That is, increasing the temperature if half cell, leads to a rise in electrode potential.

  Antoine · 1 · Apr 29 2015

• How do cells generate an electrochemical gradient?
• How do electrochemical cells produce voltage?
• How do you calculate electrochemical cell potential?
• What factors affect electrochemical cells?
• What is an electrochemical cell that generates electrical energy?
• How can I use the Nernst equation to calculate the free energy change for oxidation reduction reactions?
• What is the Nernst equation?
• What are some common mistakes students make with the Nernst equation?
• What are some examples of electrochemical processes?
• How does pH affect the Nernst equation?
• How does temperature affect the Nernst equation?
• How can I solve the Nernst equation?
• Is corrosion an electrochemical process?
• Why is the Nernst equation important?
• Effect of concentration on electrode potential according to the Nernst equation?
• What is the Nernst potential?
• Can the Nernst equation be expressed directly in terms of concentrations?
• When using the Nernst equation when can it be directly express in terms of concentrations or activities?
• Does the Nernst equation also apply when there is a net current flow through the electrode?
• What are the Boltzmann factors?
• What is an electrochemical reaction?
• What is the electromotive force?
• Question #94f7e
• What is the Nernst equation?
• What is the Nernst equation?
• A Cu/Cu2+ concentration cell has a voltage of 0.22 V at 298K. The concentration of Cu2+ in one of the half-cells is 1.6E−3 M. What is the concentration of Cu2+ in the other half-cell?
• Question #2eac3
• Question #0529c
• Question #cde21
• Question #8e5c1
• Question #3e1de
• What is the voltage of a galvanic cell made with zinc and aluminum at standard conditions?
• Question #24d99
• Question #a4ee5
• For the reaction of #"Au"^(3+)# with #"Cl"_2#, if #["Cl"^(-)]# and #["Au"^(3+)]# were initially #"0.10 M"# and #"0.25 M"# respectively, while #P_("Cl"_2) = "0.5 bar"# initially, what is #E_(cell)#?
• Question #c9882
• Question #beb88
• Question #39e4b
• What is the standard cell potential for the reaction of silver cation with aluminum metal?
• What is the potential of the 1/2 cell #Cu^(2+)+2erightleftharpoonsCu# if #[Cu^(2+)]=0.1M?# # E^@=+0.34V#.
• What is a material that allows heat to move through it easily?
• What's the cell potential?
• Would you expect molten sodium chloride to conduct electricity? Why or why not?
• The electrical conductivity of #KI#(aq) is greater than the electrical conductivity of #H_2O#(l) because the #KI#(aq) contains mobile what?
• Question #3a73e
• Does the electrolyte in a lead acid battery bubble and then evaporate due to the the heat change associated with the electrochemical reactions in the battery or is it something else?
• What are organisms that use chemical substances as a source of energy?
• Question #9b0c6
• For the 1/2 cell #sf(MnO_4^(-)+8H^(+)+5erightleftharpoonsMn^(2+)+7H_2O)# the value of #sf(E^(@)=+1.51V)#. What is the value for E if #sf([MnO_4^(-)]=0.0001M)# and #sf([Mn^(2+)]=0.0005M)# ?
• How do you find the E_cell given standard E_cell, Molarity, and the chemical reaction equation?
• Question #c0c2e
• Question #2bd1a
• Question #0c19b
• Question #c7e45
• What is the cell potential for the reaction# Mg(s)+Fe^(2+)(aq)\rarrMg^(2+)(aq)+Fe(s)# at 47 °C when #[Fe^(2+)]#= 3.50 M and #[Mg^(2+)]#= 0.110 M?
• The following cell is operated as an electrolytic cell, using a current of 0.480 A . The volume of each solution is 100.0 mL. Electrolysis is stopped after 10.00 h , and the cell is allowed to function as a voltaic cell. What is #E_(cell)# at this point?
• Full steps of getting Nernst's equation?
• Help out with the following questions about the Nernst equation and #"NAD"^+#, cytochrome c, and #"Fe"# ions?
• Question #867f3
• What is the equation that connects pH and its effect on electric potential of an electrochemical cell?
• Calculate the amount of energy not used to produce electricity when a photon of wavelength #1*10^-12m# hits sodium metal which has a work function of 2.3eV?
• In a hydrogen/oxygen fuel cell 67.2 litres of hydrogen is consumed in 5 minutes. What electric current will be produced at #sf(0^@C)# and 1 atmosphere pressure ?
• Question #471de
• Electrolysis: #"Sn"^(2+) "||" "Br"_2# What is the reaction, determine E cell, equilibrium constant and direction of electron flow? Draw cell and label anode and cathode.
• Question #138dd
• Consider the reaction #2AgCl+Cu^(2+)rarr2AgCl+Cu#. Given that #DeltaG_("rxn")=-22.kJ#, How do you find the value for #E_(rxn)^@# ?